# Delta H reaction for the following reaction: C(s)+H2O(g)=>CO(g)+H2(g) Use the following reactions a?

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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?

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

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• 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)

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