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. |
-\(\frac{dR}{dT}\) in the rate equation refers to which of the following? |
Concentration of a reactant Decrease in concentration with time Velocity constant of reaction None of these |
Decrease in concentration with time |
-\(\frac{dR}{dT}\) in the rate equation refers to decrease in concentration with time. |