Question

To calculate the enthalpy change for the reaction, 2CO (g) + O2 (g) arrow 2 CO2 (g), you can use ΔHf0 values for each reactant and product. Which setup shows how the enthalpy change should be calculated?
Answer

ΔH0reaction = [ΔHf0 CO2(g)] + [ΔHf0 CO(g) - ΔHf0 O2(g)]

ΔH0reaction = [ΔHf0 CO2(g)] - [ΔHf0 CO(g) + ΔHf0 O2(g)]

ΔH0reaction = [ΔHf0 CO(g) + ΔHf0 O2(g)] - [ΔHf0 CO2(g)]

ΔH0reaction = [ΔHf0 CO(g) - ΔHf0 O2(g)] + [ΔHf0 CO2(g)]

Is this C?

Answer 1

In general, a change in the direction of more spread out or less useful energy is spontaneous.Answer True False

Is this false? i

Answer 2

Delta H formation = Energy input of reactants - energy output of products.

Answer 3

So it is spontaneous? I know spontaneous energy spreads out but I didnt know whether it'd be considered "less useful?"

Answer 4

mean deltaG u r asking of right

Answer 5

So would the answer to the second question be true?