SOLVED

21) Given the following rate law, how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X][Y]2 A) The rate of reaction will increase by a factor of 2. B) The rate of reaction will increase by a factor of 4. C) The rate of reaction will increase by a factor of 5. D) The rate of reaction will decrease by a factor of 2. E) The rate of reaction will remain unchanged. 22) Given the following rate law, how does the rate of reaction change if the concentration of X is doubled? Rate = k [X][Y]2 A) The rate of reaction will increase by a factor of 2. B) The rate of reaction will increase by a factor of 3. C) The rate of reaction will increase by a factor of 5. D) The rate of reaction will decrease by a factor of 2. E) The rate of reaction will remain unchanged. 23) Given the following rate law, how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X][Y] A) The rate of reaction will increase by a factor of 2. B) The rate of reaction will increase by a factor of 4. C) The rate of reaction will decrease by a factor of 3. D) The rate of reaction will decrease by a factor of 2. E) The rate of reaction will remain unchanged. 24) Given the following rate law, how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X]2[Y]3 A) The rate of reaction will increase by a factor of 5. B) The rate of reaction will increase by a factor of 2. C) the rate of reaction will increase by a factor of 8. D) The rate of reaction will increase by a factor of 3. E) The rate of reaction will remain unchanged. 25) Determine the rate law and the value of k for the following reaction using the data provided. 2 N2O5(g) → 4 NO2(g) + O2(g)[ N2O5]i (M)Initial Rate (M-1s-1) 0.0934.84 × 10-4 0.0844.37 × 10-4 0.2241.16 × 10-3 A) Rate = 5.6 × 10-2 M-1s-1[N2O5]2 B) Rate = 6.0 × 10-1 M-2s-1[N2O5]3 C) Rate = 1.6 × 10-3 M1/2s-1[N2O5]1/2 D) Rate = 1.7 × 10-2 M-1/2s-1[N2O5]3/2 E) Rate = 5.2 × 10?3 s-1[N2O5] 26) The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N2O5(g) → 4 NO2(g) + O2(g) If the rate of appearance of NO2 is equal to 0.560 mol/min at a particular moment, what is the rate of appearance of O2 at that moment? A) 0.140 mol/min B) 0.280 mol/min C) 1.12 mol/min D) 2.24 mol/min 27) The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N2O5(g) → 4 NO2(g) + O2(g) If the rate of appearance of O2 is equal to 3.00 mol/min at a particular moment, what is the rate of disappearance of N2O5 at that moment? A) 0.750 mol/min B) 1.50 mol/min C) 6.00 mol/min D) 12.0 mol/min 28) For a reaction that follows the general rate law, Rate = k[A][B]2, what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00? The rate will A) decrease by a factor of 1/25.0. B) decrease by a factor of 1/5.00. C) increase by a factor of 5.00. D) increase by a factor of 25.0. 29) For a reaction that follows the general rate law, Rate = k[A][B]2, what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00? The rate will A) decrease by a factor of 1/9.00. B) decrease by a factor of 1/3.00. C) increase by a factor of 3.00. D) increase by a factor of 9.00. 30) What is the overall reaction order for the reaction that has the rate law: Rate = k[O2] [NO ]2? A) zero order B) first order C) second order D) third order