If a volcano erupts and ejects 12.5 moles of sulfur into the atmosphere how many atoms of sulfur is this

Answer:

48 minutes

Explanation:

60 divided by 25 equals 2.4 then you times 2.4 by 20

Answer

Explanation

Given:

Mass composition: 3.758 g carbon, 0.316 g hydrogen, and 1.251 grams oxygen.

What to find:

The empirical formula for the substance.

Step-by-step solution:

The first step is to convert the number of grams of each element into moles as shown below using the molar masses of H = 1.00784 g/mol and C = 12.011 g/mol and O = 15.999 g/mol

Note: Mole = Mass/Molar mass

Moles C = 3.758g/12.011 g/mol = 0.31 mol

Moles H = 0.316g/1.00784 g/mol = 0.31 mol

Moles O = 1.251g/15.999 g/mol = 0.078 mol

Now, let's divide the number of moles of each element by the smallest number obtained:

C = 0.31/0.078 = 4

H = 0.31/0.078 = 4

O = 0.078/0.078 = 1

The empirical formula for the compound is C₄H₄O₁

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

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

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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.

Answer:

D- Br

Explanation:

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

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

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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.

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

Color of reactant. Option B is correct

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

Answer:

Explanation:

Answer to the 1st one. I have my doubts for the second one so didn't post :)