10(a). Hydrogen, H_(2) reacts with nitrogen monoxide. NO as shown below: 2H_(2)(g)+2NO(g)arrow N_(2)(g)+2H_(2)O(g) The rate equation for this reaction is: rate=k[H_(2)(g)][NO(g)]^2 The concentration of NO(g) is changed and a rate-concentration graph is plotted. 9.0 8.0 7.0 6.0 5.0 4.0 3.0 2.0 1.0 0.0 __ 7.0 0.0 2.0 2.0 30 4.05.06.07 3.0 4.0 5.0 6.0 The chemist uses H_(2)(g) of concentration 2.0times 10^-2moldm^-3 Using values from the graph, calculate the rate constant, k, for this reaction. Give your answer to two significant figures and in standard form. Show your working.

## Step 1:Identify the rate law from the given information. The rate law is provided as:### ## Step 2:From the problem, we know the concentration of is .## Step 3:We need to use the values from the rate-concentration graph for to find the rate constant . Let's assume the graph provides a specific rate for a given concentration of .## Step 4:Select a point from the graph where the concentration of and the corresponding rate are known. For instance, if the graph shows that when , the rate is .## Step 5:Substitute the known values into the rate law to solve for :### ### \(1.5 \times 10^{-4} = k (2.0 \times 10^{-2}) (0.05)^{2}\)## Step 6:Solve for :### \(k = \frac{1.5 \times 10^{-4}}{(2.0 \times 10^{-2}) (0.05)^{2}}\)## Step 7:Calculate the denominator:### \((2.0 \times 10^{-2}) (0.05)^{2} = (2.0 \times 10^{-2}) (2.5 \times 10^{-3}) = 5.0 \times 10^{-5}\)## Step 8:Divide the rate by the calculated denominator:### ## Step 9:Express in standard form and to two significant figures:###