What is the theoretical yield of C2H5S in the following reaction, given 10.68 g of methane, 70.02 g of molecular sulfur (S8) and an excess of hydrogen gas?    4CH4(g)+S8 (s)+3H2(g)---> 2CsH5S(l)+6H2S(g)

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What is the theoretical yield of C2H5S in the following reaction, given 10.68 g of methane, 70.02 g of molecular sulfur (S8) and an excess of hydrogen gas?    4CH4(g)+S8 (s)+3H2(g)---> 2CsH5S(l)+6H2S(g)

Expert Solution
Step 1: Calculation of molar mass of each compound:

Given reaction:

4 C H subscript 4 left parenthesis g right parenthesis space plus space S subscript 8 left parenthesis s right parenthesis space plus space 3 H subscript 2 left parenthesis g right parenthesis space minus negative negative greater than space 2 C subscript 2 H subscript 5 S left parenthesis l right parenthesis space plus space 6 H subscript 2 S left parenthesis g right parenthesis

Calculate the molar mass of all the reactants and products:

M o l a r space m a s s space o f space m e t h a n e space left parenthesis C H subscript 4 right parenthesis space equals space 12 space plus space 4 left parenthesis 1 right parenthesis space equals 16 space g divided by m o l
M o l a r space m a s s space o f space s u l f u r space left parenthesis S subscript 8 right parenthesis space equals space 8 space cross times space 32 space equals space 256 space g divided by m o l
M o l a r space m a s s space o f space H subscript 2 space equals space 2 left parenthesis 1 right parenthesis space equals space 2 g divided by m o l
M o l a r space m a s s space o f space C subscript 2 H subscript 5 S space equals space 2 left parenthesis 12 right parenthesis space plus space 5 left parenthesis 1 right parenthesis space plus space 32
space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space equals space 61 space g divided by m o l

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