If 10.5 g of hydrogen,H2, were mixed with 6.51 g of acetylene, C2H2, and allowed to react according to the following equation, what is the theoretical yield of ethane, C2H6, produced? If 7.00 g of ethane, C2H6, were recovered at the end of the reaction, what is the percent yield?. C2H2(g)+2H2(g)=C2H6(g)

Question

If 10.5 g of hydrogen,H2, were mixed with 6.51 g of acetylene, C2H2, and allowed to react according to the following equation, what is the theoretical yield of ethane, C2H6, produced? If 7.00 g of ethane, C2H6, were recovered at the end of the reaction, what is the percent yield?.    C2H2(g)+2H2(g)=>C2H6(g)

Dorothy · Answer

Molar mass of acetylene is 35.01 g/mol

n=6.51/35.01= 0.1859 mol of C2H2

1 mol C2H2 0.1859 mol C2H2
__________= ________________
1 mol C2H6 X mol C2H6

x= 0.1859 mol C2H6

Molar mass of ethanol is 38.06 g/mol
m=(0.1859 mol)(38.06)= 7.07 g this is theoretical yield

% yield 7.00 g/7.07g x100%= 99% this is percentage yield