Answer:25.95 grams
Step-by-step explanation:
When methane and oxygen are burned together, the chemical equation is balanced as follows:
CH4 + 2O2 -> CO2 + 2H2O
We can deduce from the equation that we make 1 mole of carbon dioxide for every 1 mole of methane that reacts. Given a volume, pressure, and temperature, we can use the ideal gas law to calculate the number of moles of methane that will react:
n = PV/RT = (2.5 atm)(5.00 L)/(0.0821 L.atm/mol.K)(298 K) = 0.590 mol CH4
We know that 0.590 mol of CO2 is created since the molar ratio of CH4 to CO2 is 1:1. We need to multiply by the molar mass of CO2 to convert moles to grams:
mass = n x M, which equals (0.590 mol)(44.01 g/mol) = 25.95 g CO2.
Therefore, approximately 25.95 grams of carbon dioxide are produced when 5.00 L of methane gas reacts completely with oxygen at a pressure of 2.5 atm and a temperature of 298 K.