The reaction of nitrogen monoxide and its rate law are shown below. the concentration of no is 0.025 m, and the concentration of h2 is 0.075 m.

2no(g)+2h2(g) > n2(g)+2h2o(g)

at a given temperature, the rate constant is 1.2 m-2 x s-1. what is the rate at this temperature for the given concentrations?

there are no multiple choice options. it's just (blank) m x s-1

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :

i'm pretty sure its b i might be wrong though!