Question

The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is completely converted to product. Consider the reaction: H2(g) + C2H4(g) → C2H6(g) If 8.150 g H2 is mixed with 9.330 g C2H4, calculate the theoretical yield (g) of C2H6 produced by the reaction.

Answer 1

Answer: 9.9 grams

Step-by-step explanation:

To calculate the moles, we use the equation:

`\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}`

a) moles of
`H_2`

`\text{Number of moles}=(8.150g)/(2g/mol)=4.08moles`

b) moles of
`C_2H_4`

`\text{Number of moles}=(9.330g)/(28g/mol)=0.33moles`

`H_2(g)+C_2H_4(g)\rightarrow C_2H_6(g)`

According to stoichiometry :

1 mole of
`C_2H_4` combine with 1 mole of
`H_2`

Thus 0.33 mole of
`C_2H_4` will combine with =
`(1)/(1)* 0.33=0.33` mole of
`H_2`

Thus
`C_2H_4` is the limiting reagent as it limits the formation of product.

As 1 mole of
`C_2H_4` give = 1 mole of
`C_2H_6`

Thus 0.33 moles of
`C_2H_4` give =
`(1)/(1)* 0.33=0.33moles` of
`C_2H_6`

Mass of
`C_2H_6=moles* {\text {Molar mass}}=0.33moles* 30g/mol=9.9g`

Thus theoretical yield (g) of
`C_2H_6` produced by the reaction is 9.9 grams