How many moles of oxygen are produced from the decomposition of 36.7 g of dinitrogen pentoxide?

2N2O5 4NO2 + O2

A. 3.19 mol
B. 0.340 mol
C. 0.170 mol
D. 5.44 mol

Hi Steve, I posted this question the other day but really don't know how to answer it. Can you walk me through it please?

mol wt of N2O5 = 108

So, 36.7g = 0.340 moles

Look at the equation. Each 2 moles of N2O5 yield 1 mole of O2.

So, you will get 0.340/2 = 0.170 moles O2

Well, well, well, looks like we have a chemistry question on our hands! Don't worry, I'm here to help you out, with a sprinkle of humor, of course!

To solve this problem, we need to use the molar mass of dinitrogen pentoxide (N2O5). So, let's grab our periodic table and calculate that molar mass.

The molar mass of N2O5 is 2(14.01 g/mol N) + 5(16.00 g/mol O) = 108.02 g/mol.

Now that we have the molar mass, we can find the number of moles in 36.7 g of dinitrogen pentoxide.

36.7 g / 108.02 g/mol = 0.3399... ≈ 0.340 mol.

Now, looking at the balanced chemical equation, we can see that for every 2 moles of N2O5 that decompose, we get 1 mole of O2.

So, if we have 0.340 mol of N2O5, we will get 0.340 mol of O2.

Therefore, the answer is (B) 0.340 mol.

Hope that clears things up for you! Keep those chemistry questions coming!

To solve this problem, we can use the concept of stoichiometry. The balanced chemical equation shows that 2 moles of N2O5 produce 1 mole of O2.

First, we need to convert the mass of dinitrogen pentoxide (N2O5) into moles. To do this, we use the molar mass of N2O5.

The molar mass of N2O5 = (2 x 14.01 g/mol) + (5 x 16.00 g/mol) = 108.02 g/mol

Now, we can calculate the number of moles of N2O5:

Moles of N2O5 = mass of N2O5 / molar mass of N2O5
Moles of N2O5 = 36.7 g / 108.02 g/mol
Moles of N2O5 ≈ 0.3396 mol

Since the ratio of N2O5 to O2 in the balanced chemical equation is 2:1, the number of moles of O2 produced will also be 0.3396 mol.

Therefore, the correct answer is approximately 0.340 mol, which corresponds to option B.

Of course! Let's step through this problem together.

To find the number of moles of oxygen produced from the decomposition of dinitrogen pentoxide (N2O5), we need to use the balanced chemical equation given:
2N2O5 → 4NO2 + O2

The equation tells us that for every 2 moles of N2O5, 1 mole of O2 is produced. We are given the mass of N2O5, which is 36.7 g.

To find the number of moles of N2O5, we can use its molar mass. The molar mass of N2O5 is calculated by adding up the atomic masses of nitrogen (N) and oxygen (O):
Molar mass of N2O5 = 2(N) + 5(O) = 2(14.01 g/mol) + 5(16.00 g/mol) = 108.02 g/mol

Next, we can use the given mass and the molar mass to calculate the number of moles of N2O5:
Number of moles of N2O5 = mass / molar mass
= 36.7 g / 108.02 g/mol
≈ 0.340 mol

According to the balanced equation, 2 moles of N2O5 yield 1 mole of O2. Therefore, we can use the mole ratio to find the number of moles of O2 produced:
Number of moles of O2 = (0.340 mol N2O5) * (1 mol O2 / 2 mol N2O5)
= 0.340 mol / 2
= 0.170 mol

So, the correct answer is C. 0.170 mol.