Given the following data for heats of reaction
N2(g) + 3H2(g) ----> 2NH3(g) H = -91.8 kJ
C(graphite) + 2H2(g) -------> CH4(g)H = -74.9kJ
H2(g) + 2C(graphite) + N2(g) --------> 2HCN(g) H = 270.3 kJ
Calculate H for the reaction used to make HCN
CH4(g) + NH3(g) --------> HCN(g) + 3H2(g)
Lets number the reaction as 1, 2, 3, 4 from top to bottom
required reaction should be written in terms of other
reaction
This is Hess Law
required reaction can be written as:
reaction 4 = -0.5 * (reaction 1) -1 * (reaction 2) +0.5 * (reaction
3)
So, ΔHo rxn for required reaction will be:
ΔHo rxn = -0.5 * ΔHo rxn(reaction 1) -1 * ΔHo rxn(reaction 2) +0.5
* ΔHo rxn(reaction 3)
= -0.5 * (-91.8) -1 * (-74.9) +0.5 * (270.3)
= 256.0 KJ
Answer: 256.0 KJ
Given the following data for heats of reaction N2(g) + 3H2(g) ----> 2NH3(g) H = -91.8 kJ...
What is the enthalpy of the following reaction: CH4(g) + NH3(g) à HCN(g) + 3H2(g) Use the data from the following three reactions: N2(g) + 3H2(g) à 2NH3(g) DrH° = -91.8 kJ C(s) + 2H2(g) à CH4(g) DrH° = -74.9 kJ H2(g) + 2C(s) + N2(g) à 2HCN(g) DrH° = +270.3 kJ 437 kJ 150 kJ 391 kJ 287 kJ 256 kJ
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