You should have labeled this question as chemistry. We have few here who are experts in "Please Help Me".
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
Use the equation for the synthesis of hydrogen to answer the following.
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
1 answer