Answer: First, we need to use stoichiometry to determine how many moles of oxygen gas were consumed:
From the balanced equation, we can see that for every 4 moles of H2O produced, 5 moles of O2 are consumed. Therefore:
4 mol H2O × (5 mol O2 / 4 mol H2O) = 5 mol O2
So, 0.25 moles of H2O produced will require:
0.25 mol H2O × (5 mol O2 / 4 mol H2O) = 0.3125 mol O2
To convert from moles to liters, we need to use the ideal gas law:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. Rearranging the equation to solve for volume, we get:
V = nRT/P
Assuming standard temperature and pressure (STP) of 0°C and 1 atm, we can use R = 0.0821 L·atm/mol·K and P = 1 atm. Substituting the values, we get:
V = (0.3125 mol)(0.0821 L·atm/mol·K)(273 K) / (1 atm) = 6.62 L
Therefore, the answer is not one of the given options. The correct answer is approximately 6.62 L of oxygen gas consumed.
Step-by-step explanation: