Question

1. From the following heats of reactions that are given:
C(s) + O2 (g) --> CO2 (g) H = -393.5 kJ
2H2 (g) + O2 (g)--> 2H2O (l) H = -571.6 kJ
2C2H2 (g) + 5 O2 (g) --> 4CO2 (g) + 2H2O (l) H = -2598.8 kJ
Calculate the heat of the reaction of the following equation:
2C(s) + H2 (g) --> C2H2 (g)


2. Calculate the Hrxn for the following reaction:
2Al(s) + Fe2O3(s) --> 2Fe (s) + Al2O3(s)
Given that:
I. 2Al2O3 (s) --> 4Al (s) + 3O2(g) H= + 3339.6kJ
II. 4Fe(s) + 3O2(g) --> 2 Fe2O3(s) H= - 1644.4kJ


3. Nitrogen can exists as N2O, NH3, NO and NO2. In which compound is nitrogen in its
lowest oxidation state?

Answer 1

Answer on Question# 57952 - Chemistry - Inorganic Chemistry

1. From the following heats of reactions that are given: C(s) + O2 (g) --> CO2 (g) ΔH = -393.5 kJ

2H2 (g) + O2 (g)--> 2H2O (l) ΔH = -571.6 kJ

2C2H2 (g) + 5 O2 (g) --> 4CO2 (g) + 2H2O (l) ΔH = -2598.8 kJ

Calculate the heat of the reaction of the following equation: 2C(s) + H2 (g) --> C2H2 (g)

2. Calculate the ΔHrxn for the following reaction: 2Al(s) + Fe2O3(s) --> 2Fe (s) + Al2O3(s) Given that: I. 2Al2O3 (s) --> 4Al (s) + 3O2(g) ΔH = +3339.6kJ

II. 4Fe(s) + 3O2(g) --> 2 Fe2O3(s) ΔH = -1644.4kJ

3. Nitrogen can exist as N2O, NH3, NO and NO2. In which compound is nitrogen in its lowest oxidation state?

Solution

1.

2C(s) + H2 (g) --> C2H2 (g) ΔH = 2ΔH1 + 0.5ΔH2 - 0.5ΔH3

ΔH = 2(-393.5) + 0.5(-571.6) - 0.5(-2598.8) = 226.6 kJ

2.

2Al(s) + Fe2O3(s) --> 2Fe (s) + Al2O3(s) ΔH = 0.5ΔH1 - 0.5ΔH2

ΔH = 0.5(3339.6) - 0.5(-1644.4) = 2492 kJ

3.

The lowest oxidation state of Nitrogen is in ammonia.

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