For the hypothetical reaction 2A + B --> 3C + D, the rate was determined to be: rate = k[A]3[B]1.
What is the order of reaction with respect to A? _______
with respect to B? _______
What is the overall order of the reaction? __________
For the hypothetical reaction 2A + B --> 3C + D, the rate was determined to...
For the reaction A + 2B + 3C + D → products, the rate law is: rate =k[A][B][C] Which of the following statements are false? Select one: a. the reaction is first order in [A] b. the reaction is first order in [B] c. the reaction is first order in [D] d. the reaction is second order in [C] e. the reaction is 4th order overall Which of the following states is false? Select one: a. Catalysts provide an alternative...
Reaction 2A + B --> 3C is first order in B and zero order in A. The initial concentrations are 0.250M for A and B and 0.000M for C. The rate constant for a certain temperature is 1.30 x 10-3 s-1. Write down the rate law for this reaction in terms of disappearance of the reactant B. Calculate reaction half-life Calculate the molarity of B after 50.0 sec. Calculate the molarity of product C after 50.0 sec. Calculate molarity of...
Consider the hypothetical reaction: 2 X + Y → Z and its general rate law Rate = k[X]m[Y]n The following data was obtained when the reaction studied at –10°C: [X], M [Y], M Rate, M/min 0.10 0.10 0.18 0.10 0.20 0.36 0.20 0.20 1.45 (a) What is the order of reaction with respect to X? (2 points) (b) What is the order of reaction with respect to Y? (2 points) (c) What is the overall order of reaction?...
For the reaction, 2A + B + 3C, rate of disappearance of A is 0.3 M/s in a certain time interval. What is the average rate of appearance of C and what is the average rate of the reaction in that time interval? OA) rate of appearance of C = 0.2 M/s rate of the reaction = 0.15 M/S OB) rate of appearance of C = 0.45 M/s rate of the reaction = 0.15 M/s OC) rate of appearance of...
For a reaction 2A + 2B rightarrow C, the order with respect to A is 2 and the order overall is 2. The rate equation is: k[A]^2 [B] k[A]^2 [B]^2 k[A]^2 [B]^1 k[A]^2 [B]^3 k[A][B]
The reaction 2A → A2 was experimentally determined to be second order with a rate constant, k, equal to 0.0265 M–1min–1. If the initial concentration of A was 5.75 M, what was the concentration of A (in M) after 180.0 min?
The reaction 2A → A2 was experimentally determined to be second order with a rate constant, k, equal to 0.0265 M–1min–1. If the initial concentration of A was 3.00 M, what was the concentration of A (in M) after 180.0 min? M ?
Calculate the entropy change of the following reaction (in J/K) 2A + 2B 3C D goesn the following standard e ntropy values (given in J/mol-K): A 432.6, B 820.0, C 386.6, D 168.4 Number J/ K
Consider the following mechanism. step 1 2A > B slow B+ C D fast step 2 overall: 2A+C D Determine the rate law for the overall reaction (where the overall rate constant is represented as k) rate=
Consider the reaction: 3A + 2B ---> 2C + D Run [A] [B] Rate (M/ms) 1 100 100 6.00E+3 2 200 300 144.00E+3 3 100 200 12E+3 Determine the rate expression and overall order for the above reaction. Order with respect to B, given that A is constant should be 1 as doubling the concentration of B (runs 1 and 3) results in a doubling of the rate. Order with respect to A should be 2 as the reaction rate...