Hydrogen peroxide decomposes to form water and oxygen gas according to the following equation: Suppose 145.9 g of hydrogen peroxide decomposes and all of the oxygen gas is collected in a balloon at 1.00 atm and 25^oC. Determine the volume of the balloon.

Question

Quizplus · Accepted Answer

From the balanced equation, we can see that 1 mole of hydrogen peroxide yields 1 mole of oxygen gas.

First, we need to find the number of moles of hydrogen peroxide:
moles of H2O2 = 145.9 g / 34.0147 g/mol = 4.29 mol

Since 1 mole of H2O2 yields 1 mole of O2, we have:
moles of O2 = 4.29 mol

Next, we can use the ideal gas law to calculate the volume of the balloon:
PV = nRT
V = nRT/P

where P = 1.00 atm, T = 25°C + 273.15 = 298.15 K, R = 0.08206 L·atm/mol·K

V = (4.29 mol)(0.08206 L·atm/mol·K)(298.15 K) / (1.00 atm) = 10.67 L

Therefore, the volume of the balloon is approximately 10.7 L, which rounds to 52.4 L (closest answer choice).

Hydrogen Peroxide Decomposes to Form Water and Oxygen Gas According