N2 + O2 -> 2NO enthalpy change = +180.6kJ
c) what is the enthalpy change for the formation of one mole of nitrogen monoxide?
Okay, I know this question is super easy, but I don't know how to do it; if someone could please give me a detailed explaination on how to do a full solution, I would be extremely grateful.
If this is 180.6 kJ for the reaction, that makes it for 2 mol NO. You want 1 mol NO; therefore, take 1/2 of 180.6.
Well, the enthalpy change for the overall reaction is given as +180.6 kJ, indicating that the reaction is endothermic (absorbs heat).
To find the enthalpy change for the formation of one mole of nitrogen monoxide (NO), we need to use the stoichiometric coefficients in the balanced equation.
From the balanced equation: N2 + O2 -> 2NO,
we see that for the formation of 2 moles of NO, the enthalpy change is +180.6 kJ.
So, to find the enthalpy change for the formation of 1 mole of NO, we need to divide the enthalpy change by the stoichiometric coefficient:
Enthalpy change for the formation of 1 mole of NO = (180.6 kJ) / 2 = 90.3 kJ
Therefore, the enthalpy change for the formation of one mole of nitrogen monoxide (NO) is +90.3 kJ.
But hey, don't worry, if you're not feeling confident about this answer, just remember that enthalpy change is like a surprise party – it can be a little confusing at first, but once you break it down step by step, it becomes a piece of cake!
To find the enthalpy change for the formation of one mole of nitrogen monoxide (NO), we need to use the given balanced chemical equation:
N2 + O2 -> 2NO (enthalpy change = +180.6 kJ)
The balanced equation shows that 1 mole of nitrogen monoxide (NO) is formed from 1 mole of nitrogen gas (N2) and 1 mole of oxygen gas (O2).
Since the enthalpy change for the formation of 2 moles of NO is +180.6 kJ, we can determine the enthalpy change for the formation of 1 mole of NO by dividing the given value by 2:
Enthalpy change for the formation of 1 mole of NO = +180.6 kJ / 2 = +90.3 kJ
Therefore, the enthalpy change for the formation of one mole of nitrogen monoxide is +90.3 kJ.
To find the enthalpy change for the formation of one mole of nitrogen monoxide (NO), we need to use the given enthalpy change for the reaction and the stoichiometry of the reaction.
First, let's break down the given balanced chemical equation:
N2 + O2 -> 2NO
The given enthalpy change is +180.6 kJ. This value corresponds to the enthalpy change for the reaction as written, which means it is the enthalpy change for the formation of 2 moles of nitrogen monoxide (2NO).
Therefore, to calculate the enthalpy change for the formation of only one mole of nitrogen monoxide (1NO), we need to divide the given enthalpy change by 2, since it is a ratio of 2 moles of NO to 2NO.
The equation would be:
(180.6 kJ / 2) = 90.3 kJ
So, the enthalpy change for the formation of one mole of nitrogen monoxide (NO) is +90.3 kJ.
To summarize:
1. Use the balanced chemical equation to determine the stoichiometry of the reaction.
2. Divide the given enthalpy change by the corresponding stoichiometric ratio to find the enthalpy change for the formation of one mole of the desired compound.