Methane gas and chlorine gas react to form hydrogen chloride gas and carbon tetrachloride gas. What volume of hydrogen chloride would be produced by this reaction if 3.16 L of chlorine were consumed at STP.
Be sure your answer has the correct number of significant digits.
Answer: Thus volume of carbon tetrachloride that would be produced is 0.788 L
Explanation:
According to ideal gas equation:
[tex]PV=nRT[/tex]
P = pressure of gas = 1 atm (at STP)
V = Volume of gas = 3.16 L
n = number of moles = ?
R = gas constant =[tex]0.0821Latm/Kmol[/tex]
T =temperature =[tex]273K=[/tex]
[tex]n=\frac{PV}{RT}[/tex]
[tex]n=\frac{1atm\times 3.16L}{0.0820 L atm/K mol\times 273K}=0.141moles[/tex]
[tex]CH_4+4Cl_2\rightarrow 4HCl+CCl_4[/tex]
According to stoichiometry:
4 moles of chlorine produces = 1 mole of carbon tetrachloride
Thus 0.141 moles of methane produces = [tex]\frac{1}{4}\times 0.141=0.0352[/tex] moles of carbon tetrachloride
volume of carbon tetrachloride =[tex]moles\times {\text {Molar volume}}=0.0352mol\times 22.4L/mol=0.788L[/tex]
Thus volume of carbon tetrachloride that would be produced is 0.788 L
