Use the equation for the synthesis of hydrogen to answer the following.

Question

C (s) + H2O (l) -> CO (g) + H2 (g)

deltaH = + 31.3 kcal/mol carbon

deltaS = +32 cal/(mol•K)

Calculate the energy change (deltaH) when 5.00 g of carbon is consumed.

Calculate the energy change (deltaH) when 2.50 moles of CO is produced.

This reaction is exothermic/endothermic.
The entropy increases/decreases in this reaction

At low temperatures this reaction is spontaneous/nonspontaneous

At high temperatures this reaction is spontaneous/nonspontaneous

Calculate the deltaG for this process at 300. K

Answer 1

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a.
31.3 kcal/mol x (5.00/12) = ? kcal

b.
31.3 kcal/mol x 2.5 mol CO = ? kcal

c.
A + dH means endothermic.
A + dS means entropy is increasing.

d.
Do e first. Then set dG to zero, substitute for dH and dS and solve for T. Remember dH is in kcal/mol while dS is in cal/mol
e.
dG = dH - TdS