please can someone help

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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?

Assume constant temperature and pressure.
Feb 7th, 2015

1. PV=nRT

 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   

n=PV/RT=184.26x202.6/8.314x10^3x260.6=0.0172 mol

So the mas of HCl=0.0172x36.46=0.628 g

2. PV=nRT

   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.

Feb 7th, 2015

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Feb 7th, 2015
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