Question

The reaction of carbon dioxide(g) with hydrogen(g) to form acetylene(g) (C2H2) and water(g) proceeds as follows: 2 CO2(g) + 5 H2(g) C2H2(g) + 4 H2O(g) When 11.1 grams of CO2(g) react with sufficient H2(g) , 5.86 kJ of energy are absorbed . What is the value of H for the chemical equation given? ΔHrxn = kJ

Answer 1

Answer: 46.5 kJ

Step-by-step explanation:

The balanced chemical reaction is:

`2CO_2(g)+5H_2(g)\rightarrow C_2H_2(g)+4H_2O`

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

given mass = 11.1 g

Molar mass = 44.01 g/mol

`\text{Number of moles of carbon dioxide}=(11.1g)/(44.01g/mol)=0.252moles`

0.252 moles of carbon dioxide react with sufficient hydrogen, energy released = 5.86 kJ

2 moles of carbon dioxide react with sufficient hydrogen, energy released =
`(5.86 kJ)/(0.252)* 2=46.5kJ`

Thus value of ΔHrxn for the chemical equation given is 46.5 kJ