Answer:
5.546262 x 10^24 formula units
Explanation:
Use avogadro's number
9.21 mol CaO ((6.022 x 10^23 formula units CaO)/1 mol CaO)) = 5.546 x 10^24.
I rounded to 3 sig figs.
Which of the following will not affect the rate of a reaction?nature of the reactantscolor of reactanttemperatureconcentration of a reactant
Color of reactant. Option B is correct
Explanations:What is a rate of reactions?This is defined as the speed at which a reaction takes place. It can be expressed in terms of the concentration of reactants or products formed per unit time.
The following are the factors that affects reaction rate.
- concentration of a reactant
- Temperature
- Nature of the reactant
- Surface Area
- Catalysts.
Based on the explanations above, we can conclude that the color of reactant will not affect the rate of a reaction
What is the total pressure in kPa exerted by a mixture containing two gases if the partial pressure of one gas is 64 kPa and the partial pressure of the other gas is 50.8 kPa?
Dalton's Law or Law of Partial Pressures says that the total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas that composes it. The partial pressure of a gas on the other hand is defined as the pressure it would exert if it were alone in the container.
So we need to sum all the values:
64 + 50.8 = 114.8 kPa
Answer: 114.8 kPa
Which of the following is an element located in group 17?
a) Ne
b) Li
c) Mn
d) Br
Answer:
D- Br
Explanation:
3. 135 g of ice is placed in a beaker of water. The water temperature in the beaker is 67 °C. After all the icemelts, the final water temperature in the beaker is 19.7 °C. 4 ptsHeat of fusion for water = 334 J/g. Specific heat of water = 4.184 J/g °C. T2-T1 = 47.3 °C.Note there are a couple different ways to solve this problems to sove this por(a) Determine the initial volume of water in the beaker (before the ice was added).(b) Determine the final volume of water in the beaker (after all the ice has melted).
Answer:
Explanation:
Answer to the 1st one. I have my doubts for the second one so didn't post :)
A bike rides at an average speed of 25 km/h. How many minutes will it take for this rider to ride a distance of 20 km?
Answer:
48 minutes
Explanation:
60 divided by 25 equals 2.4 then you times 2.4 by 20
number of litres of gas in 4.51 mol Xe
First, we assume STP conditions and Ideal gas conditions.
In STP conditions, we say that:
1 mol of any gas = 22.4 L (liters)
Procedure:
1 mol Xe ------ 22.4 L (STP)
4.51 moles Xe ------- X
X = 101 L
Answer: 101 L
Which equation is balanced?
O 2Fe +02 → 2Fe2O3
O 3Fe +302 → 3Fe2O3
O 4Fe +302 → 2Fe2O3
O Fe +0₂ Fe₂O3
Answer:
C) 4Fe + 3O2 → 2Fe2O3
Explanation:
For this question, first you would go through all the options and make sure that there is an equal amount of elements on each side.
For the first option: 2Fe +02 → 2Fe2O3
You have only 2Fe atoms and 2O atoms on your reactant side and 4Fe and 6O atoms on your product side. This is not balanced.
For option b: 3Fe +302 → 3Fe2O3
You have 3Fe and 6O atoms on your reactant side while on your product side you have 6Fe and 6O atoms. This is not balanced.
For option c: 4Fe +302 → 2Fe2O3
You have 4Fe and 6O atoms on your reactant side and 4Fe and 6O atoms on your product side. This is balanced!
For option d: Fe +0₂ → Fe₂O3
You have 1Fe and 2O atoms on your reactant side and 2Fe and 3O atoms on your product side. This is not balanced.
***Remember to multiply the subscript of an element by their coefficient (number in front of molecule) if there is any.
How do I write the Empirical Formula for: A compound composed of: 9.93% carbon, 58.6% chlorine, and 31.4% fluorine
The empirical formula for a compound composed of 9.93% carbon, 58.6% chlorine, and 31.4% fluorine is CCl₂F₂.
To write the empirical formula, let us assume that total mass of the compound is 100 g, then-
Mass of carbon = 9.93 g
Mass of chlorine = 58.6 g
Mass of fluorine = 31.4 g
We know that,
Molar mass of Carbon = 12.0 g/mol
Molar mass of Chlorine = 35.5 g/mol
Molar mass of Fluorine = 18.9 g/mol
Now, we will calculate the number of moles of each using the formula -
Number of moles = Given mass
Molar mass
Moles of Carbon = 9.93 g = 0.82 mol
12.01 g/mol
Moles of Chlorine = 58.6 g = 1.65 mol
35.5 g/mol
Moles of fluorine = 31.4 g = 1.66 mol
18.9 g/mol
Now, divide each value with the smallest amount of mole we got,
carbon = 0.82 = 1
0.82
chlorine = 1.65 = 2
0.82
fluorine = 1.66 = 2
0.82
Therefore, the empirical formula of the compound can be written as - CCl₂F₂
To learn more about empirical formula,
brainly.com/question/14044066
#SPJ1
The combustion of glucose is represented by the following balanced equation:
In order to find limiting and excess reactants, we need to first, set up the equation, and it must be properly balanced:
C6H12O6 + 6 O2 -> 6 H2O + 6 CO2
1 gram of C6H12O6
1 gram of O2
From the balanced equation, we see that the molar ratio between C6H12O6 and O2 is 1:6, this means that 1 mol of C6H12O6 will react with 6 times the number of moles of O2
Now let's find the number of moles of C6H12O6, the molar mass is 180.16g/mol
180.16 g = 1 mol
1 g = x moles
x = 0.005 moles of C6H12O6, now we will need this number of moles times 6 in order to proceed with the reaction
1 C6H12O6 = 6 O2
0.005 C6H12O6 = x O2
x = 0.03 moles of O2
And this amount of moles with the molar mass of O2, which is 32g/mol
32 g = 1 mol
x grams = 0.03 moles
x = 0.96 grams of O2 in 0.03 moles
Since we have more oxygen than what we actually need, Oxygen is in excess and C6H12O6 is the limiting reactant
what is the volume (in L) in a cylinder filled with 23.0 g of N2 gas at a temperature of 65 C and a pressure of 2.37 atm?
The volume of the cylinder filled with 23.0 g of N₂ gas at a temperature of 65 °C and a pressure of 2.37 atm is 9.6 L
Given that,
Mass of the nitrogen gas in the cylinder (m) = 23 g
Temperature (T) = 65 ℃ = 65 + 273 = 338 K
Pressure (P) = 2.37 atm
R (gas constant) = 0.082057338 L.atm.K⁻¹.mol⁻¹
In Ideal gas law or general gas equation,
PV = nRT
Number of moles in nitrogen (n) = Given mass (m) of nitrogen/ Molar mass of nitrogen
Given mass (m) = 23 g
Molar mass of Nitrogen = 28 g/mol
Number of moles of nitrogen (n) = 23 / 28 = 0.82 moles of nitrogen
PV = nRT
2.37 * V = 0.82 * 0.0821 * 338
2.37 * V = 22.75
V = 22.75 / 2.37
V = 9.6 L
To know more about Molar mass
https://brainly.com/question/22997914
#SPJ1