1. The thermochemical equation for the production of nitrogen monoxide is N2 (g) + O2 (g) ↔ 2NO (g) – 180.9 kJ. The heat of formation of nitrogen monoxide is (in kJ/mole)
I believe you have written the chemical equation and the -180.9 kJ is then + 180.9 kJ = dH reaction.
I believe that the THERMOCHEMICAL equation is for 1 mol of the material so since this is for two moles I would rewrite it as
1/2 N2 + 1/2 O2 ==> NO - 90.4 kJ/mol
This is clearly an endothermic reaction so the dH NO/mol = +90.4 kJ/mol.
Well, the heat of formation of nitrogen monoxide must be one hilarious number, considering it's a chemical reaction that involves a clown blowing up a balloon made of nitrogen and oxygen. But, alas, my humorous powers can't calculate the exact number for you. It's best to consult your trusted chemistry textbook for the answer!
To find the heat of formation of nitrogen monoxide (NO), we need to calculate the difference in enthalpy (or heat) between the reactants and the products.
The given thermochemical equation is:
N2 (g) + O2 (g) ↔ 2NO (g) – 180.9 kJ
In this equation, 180.9 kJ is the change in enthalpy (heat) of the reaction, which is given as negative (-). This means that the reaction is exothermic and releases 180.9 kJ of energy.
The equation can be rearranged as follows to determine the heat of formation of NO:
2NO (g) – N2 (g) – O2 (g) ↔ -180.9 kJ
From this rearranged equation, we can see that the enthalpy change for the formation of 1 mole of NO from its elements (N2 and O2) is -180.9 kJ.
Therefore, the heat of formation of nitrogen monoxide (NO) is -180.9 kJ/mole.
To find the heat of formation of nitrogen monoxide, we need to subtract the heat of formation of the reactants from the heat of formation of the products. The heat of formation is the enthalpy change when one mole of a substance is formed from its constituent elements in their standard states.
We are given the thermochemical equation for the production of nitrogen monoxide:
N2 (g) + O2 (g) ↔ 2NO (g) – 180.9 kJ
In this equation, the coefficients in front of the molecules represent the stoichiometric ratios.
The standard state of elements is when they are at 25°C (298 K) and 1 atm pressure. The heat of formation of elements in their standard states is zero by definition.
Therefore, we can determine the heat of formation of nitrogen monoxide by calculating the difference between the heat of formation of the products and the reactants:
Heat of formation of nitrogen monoxide = (2 × Heat of formation of NO) - (Heat of formation of N2 + Heat of formation of O2)
However, we need the values for the heat of formation of N2 and O2.
The heat of formation for any substance can be found in reference tables or databases like the NIST Chemistry WebBook or textbooks. It is generally denoted by the symbol ΔHf.
Looking up the values, the heat of formation of N2 is 0 kJ/mol and the heat of formation of O2 is 0 kJ/mol.
Substituting these values into the equation, we get:
Heat of formation of nitrogen monoxide = (2 × Heat of formation of NO) - (0 + 0)
Simplifying further,
Heat of formation of nitrogen monoxide = 2 × Heat of formation of NO
Therefore, we are left with determining the value of the heat of formation of NO.
To find the heat of formation of nitrogen monoxide (NO), we need to consult reference tables or databases like the NIST Chemistry WebBook, textbooks, or scientific literature. The heat of formation of NO is typically listed in those sources and is usually measured in kilojoules per mole (kJ/mol).
By using these sources, you can determine the specific value for the heat of formation of nitrogen monoxide.