N2 + O2 = 2NO enthalpy change = +180.6kJ

c) what is the enthalpy change for the formation of one mole of nitrogen monoxide?

d) What is the enthalpy change for the reaction of 1.000 * 10^2g of nitrogen with sufficient oxygen?

I do not understand how to calculate the above, can someone please explain me.

how to calculate enthapy change of products

To calculate the enthalpy change for the formation of one mole of nitrogen monoxide (NO), you can use the given balanced chemical equation and the provided value of enthalpy change.

The given balanced chemical equation is: N2 + O2 -> 2NO

In this reaction, the enthalpy change is given as +180.6 kJ. This value represents the enthalpy change for the reaction as written, where one mole of N2 reacts with one mole of O2 to give two moles of NO.

Since you want to find the enthalpy change for the formation of one mole of NO, you need to consider the stoichiometric coefficient of NO in the chemical equation. The stoichiometric coefficient of NO is 2, which means that two moles of NO are formed for every one mole of N2.

Therefore, to find the enthalpy change for the formation of one mole of NO, you need to divide the given enthalpy change by the stoichiometric coefficient of NO:

Enthalpy change for the formation of 1 mole of NO = (+180.6 kJ) / 2 = + 90.3 kJ

So, the enthalpy change for the formation of one mole of nitrogen monoxide is +90.3 kJ.

For part (d), to calculate the enthalpy change for the reaction of 1.000 * 10^2g of nitrogen with sufficient oxygen, you need to use the concept of molar mass and stoichiometry.

Step 1: Calculate the number of moles of nitrogen (N2) using its molar mass.

The molar mass of N2 is calculated by adding the atomic masses of nitrogen:
Molar mass of N2 = (2 * atomic mass of N) = (2 * 14.01 g/mol) = 28.02 g/mol

Number of moles of nitrogen (N2) = Mass of nitrogen (N2) / Molar mass of N2
= (1.000 * 10^2 g) / (28.02 g/mol)

Step 2: Use stoichiometry to determine the enthalpy change for the given mass of nitrogen (N2) reacting with oxygen (O2).

From the balanced chemical equation N2 + O2 -> 2NO, we know that the stoichiometric ratio between N2 and NO is 1:2.

Therefore, the enthalpy change for the given mass of nitrogen reacting with sufficient oxygen can be calculated as follows:

Enthalpy change = (Enthalpy change for the formation of 1 mole of NO) * (Number of moles of nitrogen)

Enthalpy change = (+90.3 kJ/mol) * (Number of moles of nitrogen)
= (+90.3 kJ/mol) * [(1.000 * 10^2 g) / (28.02 g/mol)]

After performing the necessary calculations, you will get the enthalpy change for the reaction of 1.000 * 10^2g nitrogen with sufficient oxygen.