# Problem: Experiments were conducted to study the rate of the reaction represented by this equation.[2] 2 NO(g) + 2 H2(g) ⟶ N2(g) + 2 H2O(g) Initial concentrations and rates of reaction are given here.Consider the following questions:(d) For experiment 2, calculate the concentration of NO remaining when exactly one-half of the original amount of H2 had been consumed.

###### FREE Expert Solution

We’re being asked to calculate the concentration of NO remaining when exactly one-half of the original amount of H2 had been consumed.

Recall that the rate law only focuses on the reactant concentrations and has a general form of:

k = rate constant
A & B = reactants
x & y = reactant orders

We are going to do the following steps to solve this problem:

Step 1: Calculate the order of the reaction with respect to NO

Step 2: Calculate the order of the reaction with respect to H2

Step 3: Calculate the value of the rate constant

Step 4: Calculate the concentration of NO remaining

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###### Problem Details

Experiments were conducted to study the rate of the reaction represented by this equation.[2]
2 NO(g) + 2 H2(g) ⟶ N2(g) + 2 H2O(g)
Initial concentrations and rates of reaction are given here.

Consider the following questions:

(d) For experiment 2, calculate the concentration of NO remaining when exactly one-half of the original amount of H2 had been consumed.