The role of the force of gravity and/or fusion force in the formation of new stars form from a hydrogen and dust cloud is by providing the required force and conditions needed for the reaction.
What is a Star?This is referred to as an astronomical object which has a luminous spheroid of plasma which is held together by its gravity.
In the formation of stars, the fusion force helps in the initiation of the nucleosynthesis reaction which occurs. The outward pressure from heating of the gas must balance gravity for a new star to be formed thereby making it the correct choice.
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A quantity of 3.30 × 102 mL of 0.500 M HNO3 is mixed with 3.30 × 102 mL of 0.250 M Ba(OH)2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at 18.46°C. The heat of neutralization when 1.00 mol of HNO3 reacts with 0.500 mol Ba(OH)2 is −56.2 kJ/mol. Assume that the densities and specific heats of the solution are the same as for water (1.00 g/mL and 4.184 J/g · °C, respectively). What is the final temperature of the solution?
The final temperature of the solution is 20 °C.
Given that :
volume of HNO₃ = 0.33 L
molarity = 0.500 M
no. of moles HNO₃ = 0.33 × 0.500
= 0.165 mol
moles of Ba(OH)₂ = 0.33 × 0.250
= 0.082 mol
Q = ΔH × n
Q = - 52600 J/mol × 0.165 mol
Q = - 8679 J
total volume = 330 mL +330 mL = 660 mL
Density = mass / volume
mass = 1 g/mL × 660 mL
mass = 660 g/mL
now, the change in temperature can be calculated by following formula :
Q = mc ( ΔT )
Q = mc ( T2 - T1 )
- 8679 = 660× 4.184 ( T2 - 18.46 °C)
T2 = 20 °C
Thus, A quantity of 3.30 × 10² mL of 0.500 M HNO3 is mixed with 3.30 × 10² mL of 0.250 M Ba(OH)₂ in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at 18.46°C. The heat of neutralization when 1.00 mol of HNO₃ reacts with 0.500 mol Ba(OH)₂ is −56.2 kJ/mol. Assume that the densities and specific heats of the solution are the same as for water (1.00 g/mL and 4.184 J/g · °C, respectively). the final temperature of the solution is 20 °C.
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Can someone help me with this pls 2. Which is the volume of 3.20 moles of O₂?7. Which is the volume of 100. of O₂?
2. Which is the volume of 3.20 moles of O₂?
We are told that at STP one mol of any gas occupies 22.4 L. We will use that relationship to find the volume occupied by 3.20 moles of O₂.
1 mol of O₂ = 22.4 L
volume of O₂ = 3.20 moles of O₂ * 22.4 L/(1 mol of O₂)
volume of O₂ = 71.7 L
Answer: 3.20 moles of O₂ occupies 71.7 L
7. Which is the volume of 100. g of O₂?
In this case we will use the same relationship, but we are given grams instead of moles. So first we have to convert the mass in grams into moles. To do that we use the molar mass of O₂.
atomic mass of O = 16.00 amu
molar mass of O₂ = 2 * 16.00
molar mass of O₂ = 32.00 g/mol
Once that we know that the mass of 1 mol of O₂ is 32.00 g, we can find the number of moles that we have in 100. g of it.
moles of O₂ = mass of O₂ /(molar mass of O₂)
moles of O₂ = 100. g/(32.00 g/mol)
moles of O₂ = 3.13 moles
Finally we can find the volume that 3.13 moles of O₂ occupies (remember that 1 mol of any gas occupies 22.4 L at STP).
volume of O₂ = 3.13 moles * 22.4 L/(1 mol)
volume of O₂ = 70.1 L
Answer: 100. g of O₂ occupies 70.1 L
I need help on balancing the equations and on what type of reaction it is.
Given the balanced chemical reaction expressed as:
[tex]2Au_2O_3\rightarrow4Au+3O_2[/tex]A Redox reaction is a reaction that involves the transfer of electrons and changes in the oxidation state between the elements.
The given chemical equation is therefore an oxidation-reduction reaction since it involves a change in the oxidation state of the elements.
Determine the moles of Au₂O₃
[tex]\begin{gathered} \text{Mole = }\frac{Mass}{Molar\text{ mass}} \\ \text{Mole of Au}_2O_3=\frac{10g}{441.93g\text{/mol}} \\ \text{Mole of Au}_2O_3=0.02263\text{moles} \end{gathered}[/tex]According to stochiometry, you can see that 2 moles of Gold(III)oxide produce 4 moles of Gold. Hence the moles of Gold produced will be:
[tex]\begin{gathered} \text{moles of Gold=}\frac{0.02263\times4}{2} \\ \text{moles of Gold=}0.02263\times2 \\ \text{moles of Gold=}0.0453\text{moles} \end{gathered}[/tex]Determine the mass of Gold.
[tex]\begin{gathered} \text{Mass of Gold=moles}\times molar\text{ mass} \\ \text{Mass of Gold=}0.0453\times196.97 \\ \text{Mass of Gold}=8.91\text{grams} \end{gathered}[/tex]Next is determining the mole of Oxygen
According to stochiometry, you can see that 2 moles of Gold(III)oxide produce 3 moles of Oxygen. Hence the moles of Oxygen produced will be:
[tex]\begin{gathered} \text{moles of Oxygen=}\frac{0.02263\times3}{2} \\ \text{moles of Oxygen}=0.033945\text{moles} \end{gathered}[/tex]Determine the mass of oxygen produced
[tex]\begin{gathered} \text{Mass of O}_2=moles\times\text{Molar mass} \\ \text{Mass of O}_2=0.033945\times16 \\ \text{Mass of O}_2=0.543\text{grams} \end{gathered}[/tex]Hence the mass of oxygen produced is 0.543 grams
. At standard pressure, what state of matter is xenon at -111 °C?
A) solid
B) liquid
C) gas
D) can be both solid and liquid
E) can be both liquid and gas
At standard pressure, C) gas state of matter is xenon at -111 °C
What is the state of matter of xenon?Xenon is an extremely uncommon, odourless, colourless, tasteless, chemically inert gas. It was thought to be absolutely innocuous until Neil Bartlett published the synthesis of xenon haxafluoroplatinate in 1962. When stimulated by an electrical discharge, xenon generates blue light in a gas-filled tube.
Noble gases, which are most commonly encountered as monatomic gases, have entirely filled outer electron shells and hence have little desire to react with other elements, resulting in relatively few compounds with other elements.
In its +6 oxidation state, xenon trioxide is an unstable molecule. It is a highly potent oxidising agent that progressively liberates oxygen from water when exposed to sunshine. When it comes into touch with organic materials, it becomes highly explosive.
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Express the following in liters at STP:
4.83 x 10^-3 moles HF
Considering the definition of STP conditions, 4.83 × 10⁻³ moles of HF will occupy a volume of 0.108192 L at STP.
STP conditionsThe STP conditions refer to the standard temperature and pressure. Pressure values at 1 atmosphere and temperature at 0 ° C are used and are reference values for gases, and 1 mole of any gas occupies an approximate volume of 22.4 liters.
Volume in this caseIn this case, you have 4.83×10⁻³ moles of HF. You can apply the following rule of three: if by definition of STP conditions 1 mole of HF occupies a volume of 22.4 liters, 4.83×10⁻³ moles occupies how much volume?
volume= (4.83×10⁻³ moles ×22.4 L)÷ 1 mole
volume= 0.108192 L
Finally, there is a volume of 0.108192 L at STP.
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PLS HELP, IT’S DUE TODAY
In a nuclear fusion reaction, two small, light ___ (hydrogen atoms) combine under extreme __ and pressure to form one larger, heavier nucleus (helium).
Answer:
In a nuclear fusion reaction, two small, light 'nuclei' (hydrogen atoms) combine under extreme 'temperature' and pressure to form one larger, heavier nucleus (helium).
Calculate the boiling point of a 0.33 m solution of a solute in benzene.
(Kb = 2.53°C /m).
The boiling point of the solution is 80.93°C.
What is the boiling point?We know that the boiling point has to do with the temperature at which the pressure inside the system is the same as the atmospheric pressure. Now we know that the boiling point of the pure benzene is 80.1 °C.
Also;
ΔT = K m i
ΔT = boiling point elevation
K = boiling point constant
m = molality
i = Van Hoff factor
ΔT = 2.53°C /m * 0.33 m * 1
ΔT = 0.83°C
Boiling point of the solution = 0.83°C + 80.1 °C
= 80.93°C
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An experiment was designed to test the hypothesis that peanuts have more energy than a chip. The experiment determines calorimetry of the peanut and the chip, using water to capture the energy of the samples when they were burned. A 10 g sample of chip and a 15 g sample of peanut was burned underneath a metal can that held 50 g of water. A thermometer captured how much the temperature of the water increased. The water increased by 7 degrees for the peanut and 3 degrees for the chip. What error was made?
a The temperatures were read wrong.
b Different amounts of food samples were used.
c The food samples were too similar.
d Different amounts of water were used.
Answer:
b Different amounts of food samples were used.
Explanation:
The mass of the two samples needs to be the same in order for the test to be accurate.
When something heat up new energy is created and when something coole dan energy isdestroyer check one)How could you revise this statement to be more complete or correol?
When something heats up energy is absorbed from another system and when something cooler down energy is released to another system.
When a reaction releases heat, it is classified as exothermic. The absorption of heat in a reaction makes it endothermic.
Which naturally occurring gas can be found in certain rocks and soils and is considered a hazardous air pollutant?A. argonB. carbon dioxideC. radonD. mercury
Radon is a naturally-occuring radioactive gas that can cause lung cancer to those who are near it. Radon is also an inert, colorless and odorless gas. Although it is dangerous and hazardous, it disperses rapidly and, usually, is not a health issue. Answer is Radon
17) Which atom has a higher electronegativity, Be or O?
A redox reaction:A. is a reaction where oxygen is returned it its natural state.B. is a reduction reaction where oxygen is removed.C. is comprised of two half reactions, a reduction and an oxidation.D. is a reaction where oxygen is added to a compound.
In this question, we have to classify what is a redox reaction, and as the name suggests, we have a reduction and an oxidation reaction occurring in this type of reaction, where one element will lose electrons, or will be oxidized, and another element will gain electrons or will be reduced. Therefore the best answer will be letter C
SYNTHESIS OFCARBONATECTIONLABORATORY SIMULATIONLab Data- X99.00.10CollectedVolume sodium carbonate (mL)Molarity sodium carbonate (M)Volume calcium chloride (mL)Molarity calcium chloride (M)ObservationsThe mixture has now turned white100.00.20hemDisp0.211.30Mass filter paper (9)Mass filter paper + precipitate (9)CalculatedObserved mass calcium carbonate (9)Identify limiting reactantExpected mass calcium carbonate (9)Percent yield (%)0.88Calcium chlorideHow to calculate theoretical yield and percent yield
Answer:
[tex]\begin{gathered} \text{Limiting Reagent = Sodium Carbonate} \\ \text{Percent Yield = 98\%} \end{gathered}[/tex]Explanation:
The chemical reaction talks about the synthesis of calcium carbonate
It is from the reaction between sodium carbonate and calcium chloride
Let us write the equation of reaction as follows:
[tex]Na_2CO_{3(aq)}+CaCl_{2(aq)}\text{ }\rightarrow2NaCl_{(s)\text{ }}+CaCO_{3(aq)}[/tex]Firstly, we want to get the expected mass of calcium carbonate
This speaks about getting the theoretical yield based on the equation of reaction
From the data collected, 90 ml of 0.20 M (mol/L) of sodium carbonate gave calcium carbonate
We need to get the actual number of moles of sodium carbonate that reacted
We can get this by multiplying the volume by the molarity (kindly note that we have to convert the volume to Liters by dividing by 1000)
Thus, we have it as:
[tex]\frac{90}{1000}\times\text{ 0.1 = 0.009 moles}[/tex]Hence, we see that 0.009 moles of sodium carbonate reacted theoretically
Since 1 mole of sodium carbonate gave 1 mole calcium carbonate, it is expected that 0.009 mole of sodium carbonate will give 0.009mole of calcium carbonate
What we have to do now is to get the theoretical grams of calcium carbonate produced
That would be the product of the number of moles of calcium carbonate and its molar mass
The molar mass of calcium carbonate is 100 g/mol
The theoretical yield (expected mass) is thus:
[tex]100\text{ g/ mol }\times\text{ 0.009mol = 0.9 g}[/tex]Finally, we proceed to get the percentage yield which is calculated using the formula below:
[tex]\text{Percent Yield = }\frac{Actual\text{ yield}}{\text{Theoretical yield}}\times\text{ 100 \%}[/tex]The actual yield is the observed mass which is given as 0.88 g
The percent yield is thus:
[tex]\frac{0.88}{0.9}\times\text{ 100 = }98\text{ \%}[/tex]
why show you heat the sample to constant mass
Heating to constant mass is done to retain the constant mass of the sample so that its weight remains the same and does not affect the reading throughout the experiment.
Heating to constant mass is a process in which a sample usually a powder or crystal is heated until the mass of the sample remains constant or the same.This is done to remove the excess moisture or other impurities that may affect the accuracy of the readings during the experiment.In this process, the sample is heated, cooled down weighed, and again the sample is heated, cooled down, and weighed. This process is done repeatedly until the mass of the sample remains constant in two or three consecutive measurements. Thus, heating to constant mass gives a minimized error during the experiment.To learn more about how the mass number is calculated for an element click below:
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A legend is a traditional story that explains something in real life. Sometimes they are accepted as true, but sometimes they are fantastical and just plain fun. There are many legends that surround the North Star explaining its creation as well as why it is stationary.
Take some time to research some of the legends of the North Star. After you have had a chance to read several of them, create your own fantastical story of the North Star. It can be how it came to be or explain why it is stationary.
There are many legends of the North Star that have been told over the years by different civilizations and of them is a mythical story told about the existence of the star.
What is a Legend of the North Star?It is said that it is a little dot left behind after God created the stars and based on the fact that the dot was not like the other stars as it was almost an afterthought and then it came to the attention of Luminaria who granted the dot its wish and it became a real star like the others and became the Star of Bethlehem.
Hence, it can be seen that the given legend and mythical stories are just one of the many ways humans try to understand the phenomena of astrology and how they attach certain significance to it.
With this in mind, it is very clear to see that the North Star is a special star.
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An organic compound contains carbon hydrogen and oxygen. If it contains 45.27% carbon and 4.43 % hydrogen by mass determine the empirical formula
This organic compound has in its structure the next element: C, H, and O
45.27% C
4.43 % H
The rest 100%-45.27%-4.43 = 50.3 % O
-----------------------------------------------------------------------------------------------------------------
The empirical formula of a chemical compound is the simplest whole-number ratio of atoms present in a compound.
Procedure:
Step 1)
We convert % into grams (g). Let's assume we have a 100g sample. Therefore,
45.27 % C = 45.27 g
4.43 % H = 4.43 g
50.3 % O = 50.3 g
Step 2)
We calculate the number of moles of each element. To do this, we need every atomic mass
For C)
[tex]45.27\text{ g x }\frac{1\text{ mol}}{12.01\text{ g}}=3.767\text{ moles}[/tex]For H)
[tex]4.43\text{ g x }\frac{1\text{ mol}}{1.00\text{ g}}=\text{ 4.43 moles}[/tex]For O)
[tex]50.3\text{ g x }\frac{1\text{ mol}}{16.0\text{ g}}=3.14\text{ moles}[/tex]Step 3)
We divide all moles by the smallest one of them (3.14 moles of O)
For C) 3.767 moles/3.14 moles = 1.19 = 1 (we need integer numbers)
For H) 4.43 moles/3.14 moles = 1.41 = 1
For O) 3.14 moles/3.14moles = 1
The empirical formula is CHO
give the n and l values and the number of orbitals for sublevel 5g.
The n and l values and the number of orbitals for sublevel 5g is :
5g shell , n= 5 subshell g , l = 4, Number of orbitals for sublevel = 9.
There are total four quantum numbers:
1) Principal quantum number , n
2) Angular quantum number , l
3) Magnetic quantum number , ml
4) spin quantum number , ms
For 5g shell, n = 5
subshell g , l = 4 ....0 - s , 1 - p , 2 - d, 3 - f, 4 -g
number of orbitals in subshell = (2l + 1) ( 2×4 + 1) = 9
Thus, The n and l values and the number of orbitals for sublevel 5g is :
5g shell , n= 5 subshell g , l = 4, Number of orbitals for sublevel = 9.
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Your spaceship has docked at a space station above Mars. The temperature inside the space station is a carefully controlled 24 ∘C at a pressure of 745 mmHg . A balloon with a volume of 443 mL drifts into the airlock where the temperature is − 95 ∘C and the pressure is 0.115 atm . What is the final volume, in milliliters, of the balloon if n does not change and the balloon is very elastic?
Answer: the final volume of the balloon is 2.26 x 10^3 mL
Explanation:
The question requires us to determine the new volume of a balloon, given the initial and final conditions.
The following information was provided by the question:
initial temperature = T1 = 24 °C = 297.15 K
initial volume = V1 = 443 mL
initial pressure = P1 = 745 mmHg = 0.980 atm
final temperature = T2 = -95 °C = 178.15 K
final pressure = P2 = 0.115 atm
To solve this problem, we'll need to apply the equation of ideal gases to calculate the number of moles of gas in the balloon, and then use this value and the final temperature and pressure provided to determine the final volume,
The equation of ideal gases can be written as:
[tex]PV=nRT[/tex]And we can rearrange it to calculate the number of moles:
[tex]PV=nRT\rightarrow n=\frac{PV}{RT}[/tex]Applying the values provided by the question:
[tex]n=\frac{(0.980atm)\times(443mL)}{R\times(297.15K)}=\frac{1.46}{R}(\frac{atm\times mL}{K})[/tex]Now, we can rearrange the equation of ideal gases to calculate the volume:
[tex]PV=nRT\rightarrow V=\frac{nRT}{P}[/tex]And, applying the values provided and the number of moles as calculated:
[tex]V=\frac{(\frac{1.46}{R}atm.mL.K^{-1})\times R\times(178.15K)}{0.115atm}=2.26\times10^3mL[/tex]Therefore, the final volume of the balloon is 2.26 x 10^3 mL.
A 7.94 g of solid CO2 (Dry ice) is allowed to sublime in a balloon. The final volume of the balloon is 1.00 L at 301 K. What is the pressure?
In order to find the pressure in this situation, we will be using the Ideal gas Law, which perfectly correlates these informations, the formula for this Law is:
PV = nRT
Where:
P = pressure, we want to find it
V = volume, 1.00 L
n = number of moles, we will also find it
R = is the gas constant, 0.082
T = 301 K
To find the number of moles, we need to use the mass provided in the question and also the molar mass of CO2, 44.01g/mol
44.01g = 1 mol
7.94g = x moles
x = 0.180 moles of CO2
Now we can use the ideal gas formula:
P * 1.00 = 0.180 * 0.082 * 301
P = 4.44 atm
How many atoms of oxygen are in the reactants of the following equation? 3NO2 + H2O --> NO + 2HNO3
The reactants are the compounds before the arrow and the products are after the arrow. Just as they show us, the oxygen atoms in the reagents will bJust as the reaction shows, the oxygen atoms in the reactants will be:
Answer: There are 7 atoms of oxygen in the reactants
What change to the device would increase the amount of light energy it is converting?
A. adding magnets into the bulb
OB. increasing the size of the bulb
C. increasing the size of the vanes
D. changing the vanes to be all silver
How many significant figures (SF) are in each of the following measured quantities? Drag the appropriate measurement to the respectable bins
Chemistry => Measurements => Significant Figures
Significant figures correspond to the number of digits in a number. We have to take into account the following:
• Zeros at the beginning of a number or at the end are not counted as digits, but zeros in between the number should be counted.
,• When we write a number in scientific notation, the 10 that accompanies the number should not be counted.
Following these indications, let's count the significant figures of each given number:
In summary, we have the answer will be:
1SFs
3.00 m
4.0x10^3 mL
3SFs
50 100 00g
80.10 mL
60.4 °C
6SFs
9018.17 kg
Explain the difference between a cation and an anion. Give hints for remembering each.
Some atoms are neutral and others have positive or negative charges.
The charged atoms are called "ions".
- If the ion has positive charge, it is called cation.
- If the ion has negative charge, it is called anion.
Ions can be identified by their charge, for example:
- Cations: Na^+1, K^+1, Mg^+2
- Anions: Cl^-1, Br^-1
If you have 5.3x10^26 molecules of water how many moles of water do you have?
The question requires us to calculate the amount of moles of water that we would have in 5.3x10^26 molecules of water.
To solve this problem, we'll need to consider the Avogadro Number: this number states the amount of particles (electrons, ions, atoms, molecules etc.) in one mole of a substance. The Avogadro Number corresponds to 6.022 x 10^23 particles per mol.
Considering the Avogadro number and the number of molecules provided by the question, we can write:
6.022 x 10^23 molecules of water -------------------- 1 mol of water
5.3 x 10^26 molecules of water ------------------------ x
Solving for x, we'll have:
[tex]x=\frac{(5.3\times10^{26}molecules\text{ of water)}\times(1\text{ mol of water)}}{(6.022\times10^{23}\text{molecules of water)}}=8.8\times10^2mol\text{ of water}[/tex]Therefore, there are 8.8 x 10^2 moles of water in 5.3 x 10^26 molecules of water.
An unknown metal with a charge of 4 combines with oxygen. How many oxygen ionsare needed in a neutral compound of this metal and oxygen?
2 oxygen ions
ExplanationOxygen is a non-metal with an atomic number of 8. The electronic configuraton of the element is given as:
[tex]O;\text{ }1s^22s^22p^^4[/tex]If a an unknown metal with a charge of 4 combines with oxygen, the required reaction will be:
[tex]M^{4+}+O^{2-}\rightarrow MO_2[/tex]Since oxygen is in group VI of the periodic table and has a oxidation number of -2, to form a neutral compound with charge of +4, this means that 2 oxygen ion will combine with the metal to form a neural compound MO2
metal oxide MO2 reacts with excess HCl to produce chlorine gas at STP as given by the following unbalanced equation:MO2 (s) + HCl (aq) -,> MCl2 (aq) + Cl2 (g) + H20 (l) a. determine limiting reactantb. calculate the mass of MCl2 produced in the reactionc. calculate the percentage yield if the actual mass of MCl2 produced is 0.078g
1st) It is necessary to balance the chemical equation:
[tex]MO_2+4\text{HCl}\rightarrow MCl_2+Cl_2+2H_2O[/tex]2nd)
I’m getting certain numbers but I want to be sure I’m doing this right
To write the numbers with the specific number of significant figures, we need to remember that zeros to the left don't count as a significant figure and also that we can add zeros to the right to add significant figures to the numbers.
1) 1.5408 to 3 significant figures, we start counting from left to right, so we will maintain the numbers until the second decimal place, the "8". Since the next is "0", the rounding is "8", so the number is 1.54.
2) Here is similar, but since we don't have decimal places, we need to put the zeros in place of the numbers we are rounding. Since we want 2 significant figures, we will maintain only the first two. However, since the third is greater than 5, we need to round up, so the number is 4400.
3) To get this, we will maintain the zeros to the elft, but they don't count, so we start counting from the "1". Since the third number is less than 5, we round down, so the number is 0.019.
4) Now, here we have an example we need to add zeros. The way it is, 0.5 has only 1 significant figure, so we need to add 3 more zeros to the right to get to 4 significant figures. The number is 0.5000.
5) Here, is the same as item 3, but we want 3 significant figures and since the fourth is greater than 5 we round it up. So, the number is 0.066.
What is the MOST likely reason a large retailer would have a digital forensics lab?
A.
to investigate online shopping fraud
B.
to hack into their customers’ computers
C.
to find out who is shoplifting in their stores
D.
to help local communities solve major crimes
Answer:
A
Explanation:
In-house forensics allows companies to work faster, cheaper, and potentially better than law enforcement. Labs at large companies are more likely than police labs to have high-tech tools and the latest forensics software, said Seigfried-Spellar.
Which statement describes an intensive property of matter?
OIt is the same for every sample of a single substance.
OIt depends on how a substance was formed.
It is the same for every sample of every substance.
OIt depends on the amount of substance present.
27
It is the same for every sample of every substance present describes an intensive property of matter.
The correct option is C.
What is the meaning of intensive property?An intense property is a greater stability of a system that is independent of the system's size or the volume of its constituent elements. Based on the definitions, internal energy, volume, or density are extensive properties while pressure, temperature, and densities are intensive properties.
Why density is a intensive property?Because of the small range of densities present among the samples, density is an intense attribute. Concentrations were roughly the same regardless of the beginning mass. The data show that density is an intense attribute of matter because it is independent of the amount of substance present.
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The complete question is
Which statement describes an intensive property of matter?
A-It is the same for every sample of a single substance.
B-It depends on how a substance was formed.
C-It is the same for every sample of every substance.
D-It depends on the amount of substance present.
What is the correct formula that wouldresult from the combination of the twoionic species?Na¹+ and CIO ¹-1-4BNa₂(CIO4)2NaCIO4
To determine how the formula will be when combining two ionic species, we must look at the oxidation states of the ions. The Na ion has an oxidation state of +1 and the ClO4 ion has an oxidation state of -1.
The number of ions must be such that the total sum of the oxidation states is zero. If we have a Na+1 ion and a ClO4(-1) ion, the sum will be equal to zero. So there must be one ion of each species in the molecule.
[tex]Na^{+1}ClO_4^{-1}\rightarrow NaClO_4[/tex]Therefore, the answer will be: NaCIO4