Practicing Success
Rate of a reaction decreases with the passage of time as the concentration of reactants decrease. Conversely, rates generally increase when reactant concentrations increase. So, rate of a reaction depends upon the concentration of reactants. Consider a general reaction aA + bB → cC + dD where a, b, c and d are the stoichiometric coefficients of reactants and products. The rate expression for this reaction is Rate ∝ [A]x [B]y where exponents x and y may or may not be equal to the stoichiometric coefficients (a and b) of the reactants. Above equation can also be written as Rate = k [A]x [B]y -\(\frac{dR}{dT}\) = k [A]x [B]y This form of equation is known as differential rate equation, where k is a proportionality constant called rate constant. |
The rate of the elementary reaction 2NO + O2 → 2NO2 when the volume of the reaction vessel is halved, what is the change in the rate of reaction? |
It becomes eight times It becomes \(\frac{1}{8}\) of the initial rate It becomes four times It becomes \(\frac{1}{4}\) of the initial rate |
It becomes eight times |
For the elementary reaction 2NO + O2 → 2NO2 r = k [NO]2[O2]1 If volume of the vessel is halved, concentration of each reactant becomes doubled. r' = k[2NO]2[2O2]1 r' = 8r |