Question

For the balanced equation shown below, if the reaction of 0.112 grams of

H2 produces 0.745 grams of H20, what is the percent yield? Fe3O4 + 4H2 -> 3Fe

+ 4H2O

74.5%

84.5%

94.5%

092.2%

Answer 1

The answer is 74.5%.

Step-by-step explanation:

As we know that % yield=
`(actual yield)/(theoretical yield)` x 100%.

Therefore,

Step 1 Calculate Theoretical yield:

0.112
`H_(2)` x
`\frac{1 mol H_(2) }{2.016 g of H{2} }` x
`(4 mol H_(2)O )/(4 mol H_(2) )` x
`(18.02 g H_(2)O )/(1 mol H_(2)O)` = 1.001 g
`H_(2)O`

Now Step 2

% yield =
`(actual yield)/(theoretical yield)` x 100% =
`(0.745g)/(1.001g)` = 74.5%