Nitrogen in air reacts at high temperature to form no2 according to the reaction:

n2 + 2 o2 ? 2 no2

draw structures for the reactants and products indicating the number of single, double and triple bonds.

determine the ? h for the reaction using table 7.1.

[hint: one no2 has one [n-o] bond and one [n=o] bond]

a.

+115 kcal

b.

-78 kcal

c.

+78 kcal

d.

+7 kcal

e.

none of these

Consider the reaction: n2(g) + o2(g) ⇄ 2no(g) kc = 0.10 at 2000oc starting with initial concentrations of 0.040 mol/l of n2 and 0.040 mol/l of o2, calculate the equilibrium concentration of no in mol/l how would this be done?

According to le chatelier’s principle, a system in chemical equilibrium responds to stress by shifting the equilibrium in a direction that reduces the stress. normalizes the stress. increases the stress. changes the stress.

Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. in the first step, nitrogen and hydrogen react to form ammonia: (g) (g) (g) in the second step, ammonia and oxygen react to form nitric acid and water: (g) (g) (g) (g) calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen from these reactions. round your answer to the nearest .