Question

Hydrogen peroxide decomposes into water vapor and oxygen. Suppose you have 225 g of a solution that is 50% hydrogen peroxide by mass. What volume of oxygen can be produced at 25 °C and 792 torr?

Answer 1

To calculate the volume of oxygen produced, we can use the stoichiometry of the balanced chemical equation and the ideal gas law.

Step-by-step explanation:

To find the volume of oxygen produced, we can use the stoichiometry of the balanced chemical equation. From the equation 2H2O2(aq) -> 2H2O(l) + O2(g), we can see that one mole of hydrogen peroxide produces one mole of oxygen gas.

First, we need to find the moles of oxygen gas produced. To do this, we can convert the mass of hydrogen peroxide to moles using its molar mass.

Once we have the moles of oxygen, we can use the ideal gas law to find the volume of oxygen gas at 25 °C and 792 torr. The ideal gas law equation is PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin.