posted by .

calculate enthalpy of H for the reaction

N2H4(l) + 2H2O(l) -> N2(g) + 4H2)(l)

Given the reactions
N2H4(l) + O2(g) -> N2(g) + 2H2O(l) Enthalpy of H = -6.22.2 kJ

H2(g) + (1/2)O2(g) -> H2O(l) enthalpy of H = -285.8 kJ/mol

H2(g) + O2(g) -> H2O2(l) enthalpy of H = -187.8 kJ

You need to check the post carefully. The equation you want is not balanced. I think you have made two typos. I think the left H2O should be H2O2 and I think the right H2) should be H2O

You are defiantly right.
it is suppose to be 2H2O2(l) and 4H2O(l)

and the first equation is suppose to be -622.2 kJ/mol

actually they are all suppose to be kJ/mol, but that was a typo on the exercise.

For a final answer I got -818.2 kJ/mol

i used the first equation as is. then i used the second equation and multiplied it by two and then for the last equation i reversed it and also multiplied it by 2.

N2 + 2F2 ---> 2NF3 calculate the standard enthalpy

## Similar Questions

1. ### Chemistry

Hydrazine, N2H4, is a colorless liquid used in rocket fuel. What is the enthalpy change for the process in which hydranzine is formed from its elements?
2. ### chemistry

N2H4 reacts with oxygen to yield nitrogen gas and water . The reaction of 3.80g n2h4 evolves 73.7kj of heat. what's the enthalpy change per mole of hydrazine combusted.

calculate enthalpy of H for the reaction N2H4(l) + 2H2O(l) -> N2(g) + 4H2)(l) Given the reactions N2H4(l) + O2(g) -> N2(g) + 2H2O(l) Enthalpy of H = -6.22.2 kJ H2(g) + (1/2)O2(g) -> H2O(l) enthalpy of H = -285.8 kJ/mol H2(g) …
4. ### Chemistry - Science (Dr. Bob222)

Hydrazine is used as a rocket fuel because its reaction with oxygen is extremely exothermic: N2H4(liquid) + O2(g)  N2(g) + 2H2O(liquid) ΔH(reaction) = -615 kJ mol-1 What is the enthalpy of this reaction if water were produced …
5. ### Chemistry help

I am not to sure how to approach the problem... Hydrazine is used as a rocket fuel because its reaction with oxygen is extremely exothermic: N2H4(liquid) + O2(g) ==> N2(g) + 2H2O(liquid) ΔH(reaction) = -615 kJ mol-1 What is …
6. ### Chemistry

Calculate the value of the standard enthalpy change for each of the following reactions (standard enthalpy for Na2SO4(s) is -1375.653 kj/mole): a) 4HBr(g) + O2(g) = 2H2O(I) + 2Br(I) b) 2Na(OH)(s) + SO3(g) = Na2SO4(s) + H2O(g) c) CH4(g) …
7. ### Chemistry

Calculate the value of the standard enthalpy change for each of the following reactions (standard enthalpy for Na2SO4(s) is -1375.653 kj/mole): a)4HBr(g) + O2(g) = 2H2O(I) + 2Br(I) b)2Na(OH)(s) + SO3(g) = Na2SO4(s) + H2O(g) c)CH4(g) …
8. ### chemistry

The enthalpy change for the following reaction is -483.6 kJ: 2H2(g) + O2(g) = 2H2O(g) Therefore, the enthalpy change for the following reaction is _______ kJ: 4H2(g) + 2O2(g) = 4H2O(g)
9. ### chemistry

Hess¡¯ law says that when we add reactions together we can also add the enthalpies. Given the following set of reactions, use Hess¡¯ Law to calculate the enthalpy of the reaction given below. N2H4 + H2 ¡æ 2 NH3 ¥ÄH¡Æ = ?
10. ### chemistry

Calculate the value of the thermodynamic equilibrium constant for the following reactions at 25.0 °C. (a) N2H4(g) + 2O2(g) 2NO(g) + 2H2O(g) Kp = H20=-228.6 NO= 86.69 N2H4= 159.3 02 = 0

More Similar Questions