Question

1)

CH4(g)+2O2(g)→CO2(g)+2H2O(l)ΔHrxno=−889.1kJmol–1

ΔHfoH2O(l)=–285.8kJmol–1ΔHfoCO2(g)=–393.3kJmol–1

What is the standard heat of formation, ΔHfo, of methane, CH4(g), as calculated from the data above?

2)

How much heat, in kilojoules, must be added to a 75.0–g iron block with a specific heat of 0.449 J/g°C to increase its temperature from 25 °C to its melting temperature of 1535 °C?

3)

Calculate ΔH298o for the process

Sb(s)+52Cl2(g)→SbCl5(g)

from the following information:

Sb(s)+32Cl2(g)→SbCl3(g)ΔH298o=−314kJ

4)

The oxidation of the sugar glucose, C6H12O6, is described by the following equation:

C6H12O6(s)+6O2(g)⟶6CO2(g)+6H2O(l)ΔH=−2816kJ

The metabolism of glucose gives the same products, although the glucose reacts with oxygen in a series of steps in the body. How much heat in kilojoules can be produced by the metabolism of 1.0 g of glucose?

5)

Calculate ΔG° for the following reaction from the equilibrium constant at the temperature given.

HF(aq)+H2O(l)⟶H3O+(aq)+F−(aq),T=25°C,K=7.2×10−4

Please show all the step involved with formulas ! Thanks

Answer 1