N2(g) + 3H2(g) → 2NH3(g)+ 22,000 cal equals how much ΔH

convert calories to joules.

take note of the delta H for its sign.

22 kcal

To calculate the value of ΔH (the enthalpy change) for the given reaction, you need to sum up the enthalpy changes of the individual reactions of the reactants and products. The given enthalpy change of 22,000 cal represents the enthalpy change for the reaction as a whole.

The balanced chemical equation is:
N2(g) + 3H2(g) → 2NH3(g)

The enthalpy change can be determined using the enthalpy values of the reactants and products. The enthalpy values are typically given in kilojoules (kJ), so we need to convert the given value from calories (cal) to kilojoules (kJ).

1 cal = 4.184 J
1 J = 0.001 kJ

Therefore, 22,000 cal is equal to (22,000 cal) * (4.184 J/cal) * (0.001 kJ/J) = 92.048 kJ.

So, the value of ΔH for the reaction is 92.048 kJ.

To find the value of ΔH (enthalpy change) for the given reaction, you need to determine the energy change per mole of the reaction.

The equation for the reaction is:
N2(g) + 3H2(g) → 2NH3(g)

The given value of 22,000 cal represents the energy change for the reaction.

To calculate ΔH, you need to convert the given value from calories to joules, as joules are the SI unit of energy.

1 calorie (cal) = 4.184 Joules (J)

So, to convert 22,000 cal to Joules, you can use the conversion factor:

22,000 cal × 4.184 J/cal = 92,048 J

Now, you have the energy change in Joules.

Next, you need to determine the number of moles of the reaction. Comparing the balanced equation, you can see that one mole of N2 reacts with three moles of H2 to produce two moles of NH3.

From the equation, the reaction stoichiometry is 1:3:2 for N2, H2, and NH3, respectively.

Using this stoichiometry, you can calculate the number of moles of the reaction.

Since the stoichiometry of the reaction is 1:3:2, it means that for every 1 mole of N2 reacting, 3 moles of H2 are needed, resulting in 2 moles of NH3.

Now, you have a conversion factor of: 2 moles NH3 / 22,000 J

Finally, you can calculate ΔH by dividing the energy change by the number of moles of the reaction:

ΔH = Energy change / Moles of reaction
ΔH = 92,048 J / 2 moles
ΔH ≈ 46,024 J/mol

Therefore, the ΔH (enthalpy change) for the given reaction is approximately 46,024 J/mol.