What is the mass of a 202.6 mL sample of hydrogen chloride gas at -12.4oC and 184.26 kPa
2,,,What volume of water vapor is created by the complete combustion of 35.5 liters of methane gas?
V=202.6 ml, T=-12.4 C=273-12.4 K=260.6 K, P=184.26 kPa, R=8.314x10^3 cm3kPa K−1 mol−1
So the mas of HCl=0.0172x36.46=0.628 g
Assume constant temperature and pressure, so the volume of the gas is proportional to the mole of the gas.
When CH4 is completely reacted,
CH4+O2 ==== CO2 + 2H2O
So the molar ration between H2O and CH4 is 2:1, hence the volume ratio between H2O and CH4 is 2:1.
Therefore 35.5 liters of methane gas could produce 2x35.5=70.0 liters of water vapor.
Content will be erased after question is completed.
Enter the email address associated with your account, and we will email you a link to reset your password.
Forgot your password?