Calculate Delta H reaction for the following reaction:?
Calculate Delta H reaction for the following reaction: C(s)+H2O(g)=>CO(g)+H2(g) Use the following reactions a?
Please Help! I DO need the ANSWER BUT MORE IMPORTANT I need the STEPS to the Answer!
Calculate Delta H reaction for the following reaction:
C(s)+H2O(g)=>CO(g)+H2(g)
Use the following reactions and given Delta H:
C(s)+O2(g)=>CO2(g), Delta H= 393.5 kJ
2CO(g)+O2(g)=>2CO2(g) , Delta H= 566.0 kJ
2H2(g)+O2(g)=>2H2O(g) , Delta H= 483.6 kJ
Answer in 4 sig figs, for kJ
3 Answers

rearrange the second equation to obtain CO on the other side of the equation(Delta H is now reversed for that equation, 556.0kJ)
do the same for the third equation to obtain H2 on the other side; swith Delta H
Combine all three equations, and cancel like terms:
C(s)+O2(g)+2CO2(g)+2H2O(g)=CO2(g)+2CO(g)+O2(g)+2H2(g)+O2(g)
After cancelling you should get:
2C(s)+2H2O(g)=2CO(g)+2H2(g)
Add all Delta H’s(393.5+566+483.6)=656.1kJ
Because this is for 2 moles of everything, you have to half the answer:
328.1kJ

Reverse the second and third equations. After doing so change the signs of the Delta H’s of said equations. After that half the same equations.
C(s)+O2(g)==>CO2(g) Delta H = 393.5kJ
2CO(g)+O2(g)=>2CO2(g) Delta H= 566.0 kJ
2H2(g)+O2(g)=>2H2O(g) Delta H= 483.6 kJ
then becomes:
C(s)+O2(g)==>CO2(g) Delta H = 393.5kJ
CO2(g)==>CO(g)+.5O2(g) Delta H = 283.0 kJ
H2O(g)==>H2(g)+.5O2(g) Delta H = 241.8 kJ
After cancelling like terms you will end up with the target equation, C(s)+H2O(g)==>CO(g)+H2(g).
Add the Delta Hs and you’ll get 131.3 kJ

Marquise is absolutely right!!
The answer is indeed 131.3 kJ