# Chemistry II

posted by .

The value of ^G for the following reaction is -5490 kJ. Use this value and data to calculate the standard free energy of formation for C4H10 (g).

2 C4H10 (g) + 13 O2 (g) --> 8 CO2 (g) + 10 H2o (l)

Do you know the heats of formation for CO2 and H2O?

Wouldn't delta G/2, minus 4 Hfco2, minus 5 Hfh2o, equal Hfbutane?

• Chemistry II -

heat of formation for CO2(g) is -393.5 kJ/mol and for H2O(l) it's -285.8 kJ/mol

## Similar Questions

1. ### Chemistry II

The value of ^G for the following reaction is -5490 kJ. Use this value and data to calculate the standard free energy of formation for C4H10 (g). 2 C4H10 (g) + 13 O2 (g) --> 8 CO2 (g) + 10 H2o (l)
2. ### Chemistry II

The value of ^G for the following reaction is -5490 kJ. Use this value and data to calculate the standard free energy of formation for C4H10 (g). 2 C4H10 (g) + 13 O2 (g) --> 8 CO2 (g) + 10 H2o (l)
3. ### Chemistry

Balance each of the following skeleton equations. This is the last one left to balance. D) C4H10 + O2 -> CO2 + H2O = C4H10 + O2 -> 4CO2 + 10H
4. ### chemistry

Balance the equation ?C4H10 (g) + ?O2 (g) ! ?
5. ### Chemistry

For the reaction: C4H10 + O2 ¨ CO2 + H2O ( is this balanced?
6. ### Chemistry

My question is ..can anyone explain how to do problem #2?
7. ### chemistry

A method for scrubbing CO2(g) from the air on a spacecraft is to allow CO2(g) to react with NaOH according to the following (unbalanced reaction). NaOH(s) + CO2(g) → Na2CO3(s) + H2O(l) Use the appropriate thermodynamic tables …
8. ### Chemistry

Based on the following balanced equation: 2 C4H10 + 13 O2 --> 8 CO2 + 10 H2O a. How many moles of CO2 are produced after complete reaction of 8.00 moles of C4H10?
9. ### chemistry

For combustion of 10 grams of C4H10 excess of O2, You are obtained 25 grams of CO2 according to the reaction (to balance): C4H10+ O2→ CO2+ H2O Calculate the reaction yield of the reaction. please,could anyone help me to solve …
10. ### Chemistry

The enthalpy of combustion of butane C4H10 is described by the reaction: C4H10(g) + (13/2) O2(g) -> 4CO2(g) + 5H2O(g) ΔH°rxn = –2613 kJ/mol Given the following enthalpies of formation: ΔH°f[CO2(g)] = -393.5 kJ/mol ΔH°f[H2O(g)] …

More Similar Questions