Rate law for the reaction aA + bB cC + dD is r = k [ A ][ B ] . Which from following conditions does NOT affect the rate of reaction?

Step-by-step solution

The rate law for the reaction aA + bB cC + dD is given as r = k[ A ][ B ] . With initial concentrations [ A ]₀ and [ B ]₀ , the initial rate is r₀ = k[ A ]₀[ B ]₀ . Analyzing each condition: Option A: Doubling [ A ] while keeping [ B ] constant yields r_A = k(2[ A ]₀)([ B ]₀) = 2r₀ , changing the rate. Option B: Doubling [ B ] while keeping [ A ] constant gives r_B = k([ A ]₀)(2[ B ]₀) = 2r₀ , altering the rate. Option C: Halving [ A ] while doubling [ B ] results in r_C = k( 1 2 [ A ]₀)(2[ B ]₀) = r₀ , leaving the