when no(g) reacts with h₂(g) to form n₂(g) and h₂o(ℓ), 376 kj of energy are evolved for each mole of no(g)…

when no(g) reacts with h₂(g) to form n₂(g) and h₂o(ℓ), 376 kj of energy are evolved for each mole of no(g) that reacts. write a balanced thermochemical equation for the reaction with an energy term in kj as part of the equation. use the smallest integer coefficients possible. include states of matter. reactants + + products → + +

when no(g) reacts with h₂(g) to form n₂(g) and h₂o(ℓ), 376 kj of energy are evolved for each mole of no(g) that reacts. write a balanced thermochemical equation for the reaction with an energy term in kj as part of the equation. use the smallest integer coefficients possible. include states of matter. reactants + + products → + +

Answer

Explanation:

Step1: Write un - balanced equation

$NO(g)+H_2(g)\rightarrow N_2(g)+H_2O(l)$

Step2: Balance the nitrogen atoms

$2NO(g)+H_2(g)\rightarrow N_2(g)+H_2O(l)$

Step3: Balance the oxygen atoms

$2NO(g)+H_2(g)\rightarrow N_2(g)+2H_2O(l)$

Step4: Balance the hydrogen atoms

$2NO(g)+2H_2(g)\rightarrow N_2(g)+2H_2O(l)$

Step5: Determine the energy term

Since 376 kJ of energy is evolved per mole of $NO(g)$ and there are 2 moles of $NO(g)$ in the balanced equation, the total energy evolved is $2\times376 = 752$ kJ. Since energy is evolved, it is written on the product side.

Answer:

$2NO(g)+2H_2(g)\rightarrow N_2(g)+2H_2O(l)+752\ kJ$