Top topic this week
Back to FAQs
Related FAQs
Frequently Asked Question
Questions asked by users might not always be phrased in the clearest way.
Methane (ch4) reacts with oxygen gas to form carbon dioxide and water vapour in a complete hydrocarbon combustion reaction.rnrnat 21.1 oc and a pressure of 99.650 kpa, 54 l of carbon dioxide are produced. Calculate the mass (in grams) of methane required. Isn't it supposed to be 35.20g
Accepted Answer
The balanced chemical equation for the complete combustion of methane (CH4) is:
CH4 + 2O2 → CO2 + 2H2O
From the ideal gas law, we can calculate the number of moles of carbon dioxide produced:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
n = PV/RT
n = (99.650 kPa)(54 L)/(8.314 J/mol·K)(294.25 K)
n = 2.23 mol CO2
From the stoichiometry of the balanced chemical equation, we see that 1 mole of CH4 produces 1 mole of CO2. Therefore, the number of moles of CH4 required is also 2.23 mol.
The molar mass of CH4 is 16.04 g/mol. Therefore, the mass of CH4 required is:
mass = n × molar mass
mass = 2.23 mol × 16.04 g/mol
mass = 35.74 g
Therefore, the mass of methane required is 35.74 g, not 35.20 g.
Articles you might like