Consider the following chemical reaction: 2H2O(l)→2H2(g)+O2(g) What mass of H2O is required to form 1.3 L of O2 at a temperature of 295 K and a pressure of 0.926 atm ?

The mass of water required is 1.79 grams

Explanation:

To calculate the amount of oxygen gas, we use the equation given by ideal gas which follows:

where,

P = pressure of the gas = 0.926 atm

V = Volume of the gas = 1.3 L

T = Temperature of the gas = 295 K

R = Gas constant =

n = number of moles of oxygen gas = ?

Putting values in above equation, we get:

For the given chemical equation:

By Stoichiometry of the reaction:

1 mole of oxygen gas is produced from 2 moles of water

So, 0.0497 moles of oxygen gas will be produced by = of water

To calculate the number of moles, we use the equation:

Moles of water = 0.0994 moles

Molar mass of water = 18 g/mol

Putting values in above equation, we get:

Hence, the mass of water required is 1.79 grams