What is the percent yield of H2 if 58.94g of methane yields 14.61g of H2

Question

What is the percent yield of H2 if 58.94g of methane yields 14.61g of H2 for the following reaction: CH4(g) + 2H2O(g)->4 H 2 (g) + CO2(g)

Answer 1

Hi Karla, percent yield = (actual yield/ theoretical yield ) x 100

 

where:

 

actual yield is the amount of product obtained (this is experimental result), and

 

theoretical yield is the amount of product calculated based on the balanced chemical equation (this is theoretical or predicted amount).

 

Thus, 14.61 g H2 is the actual yield. 

 

To find the theoretical yield, you have to calculated the amount of H2 that will be produced from 58.96 g of methane according to the equation.

 

                 CH4(g)   +   2H2O(g)->   4 H 2 (g) +   CO2(g)

 

mol:           1 mol                              4 mol
 

gram:         16 g                                8 g          (use the molar mass to convert mol. to gram)

 

 

8 g H2 is formed from 16 g of CH4. Thus, from 58.96 g CH4

 

                                      (8 g H2/16 g CH4) x 58.96 g CH4  = 29.48 g H2 will be formed

 

 

percent yield =  (14.61 g/29.48) x 100 = 49.5 %