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Chemistry
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13 Dec 2019

) Without calculations, determine which of the following is ALWAYS spontaneous?

a) C2H6O (l) + 3 O2 (g) → 2 CO2 (g) + 3 H2O (g); ΔH < 0

b) The sublimation of dry ice (CO2 )

c) The freezing of water (H2O)

d) The formation of water from its gaseous elements

e) None of the above are ALWAYS spontaneous

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Related questions

Without doing any calculations determine what the sign of ∆S will be for the following equations.

A. 2 CO(g) + O2(g) → 2 CO2(g)

B. H2O(l) → H2O(g)

C. C5H12(g) + 8 O2(g) → 5 CO2(g) + 6 H2O(g)

Without doing calculations predict if the above reaction A is spontaneous given ∆Hrxn = -566.0kJ

Which of the following reactions is NOT spontaneous at standard state?

2Al(s) + 3/2O2(g) = Al2O3(s)

Carbon (graphite) + O2(g) = CO2(g)

Ca(s) + H2O(l) = Ca(OH)2(aq) + ½H2(g)

Any reaction with a negative ΔG value for the reaction.

All the reactions listed above are spontaneous at standard state.

Question 1

Iron is made from a reaction of iron oxide with carbon monoxide in the following reaction:

Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g)

Using Hess' Law, calculate the enthalpy of reaction given:

C(s) + O2(g) → CO2(g) ΔH = -393.5 kJ/mol

2 Fe(s) + 3/2 O2(g) → Fe2O3(s) ΔH = -824.2 kJ/mol

C(s) + 1/2 O2(g) → CO(g) ΔH = -110.5 kJ/mol

Question 2

Use Hess' Law to calculate enthalpy of reaction for the following equation:

2 N2(g) + 5 O2(g) → 2 N2O5(g)

Given:

2 H2(g) + O2(g) → 2 H2O(l) ΔH = -571.6 kJ/mol

N2O5(g) + H2O(l) → 2 HNO3(l) ΔH = -76.6 kJ/mol

1/2 N2(g) + 3/2 O2(g) + 1/2 H2(g) → HNO3(l) ΔH = -174.1 kJ/mol

Question 3

Using standard enthalpies of formation, determine the ΔHreaction for the following equations:

2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(g)

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