The enthalpy change of the reaction, ΔH = -311 kJ
Enthalpy change involved in the reaction of 300 g of CO = -10972.5 kJ
<h3>What is the enthalpy change for the reduction of ethyne to form ethane?</h3>
The enthalpy change for the reaction is obtained from the summation of the enthalpies of the reactions of the intermediate steps according to Hess's law.
The equation of the reaction is given below:
The enthalpy of the reaction, ΔH = ΔH₁ + 2ΔH₂ + (-ΔH₃)
ΔH = {(-1299) + (2 * -286) + (1560)}Kj
ΔH = -311 kJ
The equation for the methanation reaction is given below:
3 H₂O + CO → CH₄ + H₂O
The enthalpy for the methanation reaction is as follows:
ΔH = 1.5ΔH₁ + 0.5*(-ΔH₂) + ΔH₃ + -ΔH₄
ΔH = (-483.6 * 1.5) + (0.5 * 221.0) + (-802.7) + (393.5)
ΔH = -1024.1 kJ/mol
Molar mass of CO = 28 /mol
Enthalpy change involved in the reaction of 300 g of CO = 300/28 * -1024.1 kJ/mol
Enthalpy change involved in the reaction of 300 g of CO = -10972.5 kJ
In conclusion, the enthalpy changes are calculated from the enthalpy values of the intermediate reactions.
Learn more about enthalpy changes at: brainly.com/question/26991394
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