Question

Question 6 1.5 pts Predict under what temperatures (all temperatures, low temperatures, or high temperatures), if any, the following reactions will be spontaneous. A. 2CO(g) + O2(g) = 2002(g), AH rxn=-566.0 kJ [ Select] B. 2NO2(g)2NO(g)+O2(g), AH rxn= +113.1 kJ [ Select ] C. 2H2(g)+O2(g)—2H2O(g), AH rxn=-483.6 kJ [ Select] D. 2H2O2(1)→2H2O(1)+O2(g), AH rxn= -196.0 kJ [Select ]

Answer 1

3)

A)

ΔHrxn is negative

ΔSrxn is negative as there are more gases in reactant than product and hence entropy of reactant is more than that of product.

use:

ΔGrxn = ΔHrxn - T*ΔSrxn

for reaction to be spontaneous, ΔGrxn should be negative

It would be negative at low temperature

Answer: low temperatures.

B)

ΔHrxn is positive

ΔSrxn is positive as there are more gases in product than reactant and hence entropy of product is more than that of reactant.

use:

ΔGrxn = ΔHrxn - T*ΔSrxn

for reaction to be spontaneous, ΔGrxn should be negative

It would be negative at high temperature

Answer: high temperatures.

C)

ΔHrxn is negative

ΔSrxn is negative as there are more gases in reactant than product and hence entropy of reactant is more than that of product.

use:

ΔGrxn = ΔHrxn - T*ΔSrxn

for reaction to be spontaneous, ΔGrxn should be negative

It would be negative at low temperature

Answer: low temperatures.

D)

ΔHrxn is negative

ΔSrxn is positive as there are more gases in product than reactant and hence entropy of product is more than that of reactant.

use:

ΔGrxn = ΔHrxn - T*ΔSrxn

for reaction to be spontaneous, ΔGrxn should be negative

It would be negative at all temperature

Answer: all temperatures.