Calculate the mass of water and carbon monoxide (iv) that are formed during the combustion of natural gas

| June 16, 2021 | education

Calculate the mass of water and carbon monoxide (iv) that are formed during the combustion of natural gas with a volume of 1m3, if the content of methane in it is 89.6% (the rest is inorganic impurities)

1. Let’s compose the equation of the chemical reaction:

CH4 + O2 = CO2 + H2O.

2. Find the chemical amount of methane (Vm – molar volume, constant equal to 22.4 l / mol):

1 m3 = 1000 liters.

V (CH4) = V (mixture) * ω (CH4) / 100% = 1000 l * 89.6% / 100% = 896 l.

n (CH4) = V (CH4) / Vm = 896 L / 22.4 L / mol = 40 mol.

3. Using the reaction equation, we find the chemical amount of water and carbon dioxide, and then their masses:

n (H2O) = n (CH4) = 40 mol.

m (H2O) = n (H2O) * M (H2O) = 40 mol * 18 g / mol = 720 g.

n (CO2) = n (CH4) = 40 mol.

m (CO2) = n (CO2) * M (CO2) = 40 mol * 44 g / mol = 1760 g.

Answer: m (H2O) = 720 g; m (CO2) = 1760 g.



One of the components of a person's success in our time is receiving modern high-quality education, mastering the knowledge, skills and abilities necessary for life in society. A person today needs to study almost all his life, mastering everything new and new, acquiring the necessary professional qualities.