The rate equation for the gas-phase reaction between nitrogen monoxide (NO\text{NO}NO) and oxygen (O2\text{O}_2O2) is:
rate=k[NO]2[O2] \text{rate} = k[\text{NO}]^2[\text{O}_2] rate=k[NO]2[O2]State what is meant by the term overall order of reaction.
Deduce the overall effect on the rate of reaction when the concentration of NO\text{NO}NO is halved and the concentration of O2\text{O}_2O2 is multiplied by eight.
At a certain temperature, the rate of reaction is 0.0720 mol dm−3 s−10.0720\text{ mol dm}^{-3}\text{ s}^{-1}0.0720 mol dm−3 s−1 when the concentration of O2\text{O}_2O2 is 0.125 mol dm−30.125\text{ mol dm}^{-3}0.125 mol dm−3. Calculate the concentration of NO\text{NO}NO if the rate constant, kkk, is 3.60 mol−2 dm6 s−13.60\text{ mol}^{-2}\text{ dm}^6\text{ s}^{-1}3.60 mol−2 dm6 s−1.
