Find the heat of formation for a mole of hydrazine (N2H4) given: 2N2H4(l) + 2O2(

Question

Find the heat of formation for a mole of hydrazine (N2H4) given: 2N2H4(l) + 2O2(g) ? 2N2(g) + 4H2O(g) ? Ho = -1068.4 kJ H2(g) + 1/2O2(g) ? H2O(g) ? Ho = -241.8 kJ

Explanation / Answer

let 2N2H4(l) + 2O2(g) ? 2N2(g) + 4H2O(g) ? Ho = -1068.4 kJ ---> equation1 H2(g) + 1/2O2(g) ? H2O(g) ? Ho = -241.8 kJ --------> equation2 the formation of hydrazine is as below N2 + H2 --> N2H4 [ ignore first either it is balance or not ] in order to make N2H4 to become the product, we have to shift equation 1 so it will be 2N2(g) + 4H2O(g) ?2N2H4(l) + 2O2(g) ? Ho = +1068.4 kJ and the equation 2 must be multiply with 4 in order to cancel out both of the equation. the new equation will be ; 4H2(g) + 2O2(g) ? 4H2O(g) ? Ho = ( -241.8 kJ x4) so then we can cancel out H2O and O2. the remaining is 2N2 + 4H2 -----> 2N2H4 ? formation = +1068.4kJ + (-967.2kJ) = +101.2kJ hope this help :)

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