QUESTION 12 For the reaction A ® B, the rate law is A[B] - k[A]. At...
AB 3. For the reaction 2 A B , the rate law is a = k[A]. What are the units of the rate constant where time is measured in seconds? A) B) M. C) Ń D) EMS What are the units of the
QUESTION 28 The rate law of a particular reaction was determined to be Rate = k[A][B]. What is the unit of the rate constant for the reaction? a. M/s b. 1/(Ms) c. 1/(Ms2) d. 1/s e. Ms
The rate law of a particular reaction was determined to be Rate = k. What is the unit of the rate constant for the reaction? a. Ms b. M/s c. 1/s d. 1/(Ms) e. 1/(Ms2)
The reaction B ➔ products follows the rate law Rate = k [B]2. If the initial concentration of B is 0.400 M, it requires 100 seconds for [B] to fall to 0.200 M. The additional reaction time (in seconds) that is required for [B] to reach 0.100 M is A. 125 B. 175 C. 100 D. 150 E. 200
Match the descriptions to the appropriate term. Rate of reaction Rate law Rate constant Answer Bank always has units of amount per time (i.e., molarity per second, M/s, or molarity per minute, M/min) symbolized as k can have different units, such as molarity per second (M/s), inverse seconds (s-1), or inverse molarity-seconds (M-1.s-1 depending on the reaction order a formula that relates reactant concentration to reaction rate
The rate law for the reaction 2NO2 + O3 → N2O5 + O2 is rate = k[NO2][O3]. Which one of the following mechanisms is consistent with this rate law? A) NO2 + NO2 → N2O4 (fast) N2O4 + O3 → N2O5 + O2 (slow) B) NO2 + O3 → NO5 (fast) NO5 + NO5 → N2O5 + 5/2O2 (slow) C) NO2 + O3 → NO3 + O2 (slow) NO3 + NO2 → N2O5 (fast) D) NO2 + NO2 → N2O2...
Iwo experiments were performed to determine the rate law for the reaction shown below. In both experiments [A] was measured as a function of time in seconds; in experiment 1, 0.200 M B was used and in experiment 2, 0.400 M B was used. In both experiments, the graph of [A] vs time was linear; the slopes of those lines are given in the table. 4. A+B AB Exp Initial [B] (M) Slope of [A] vs time 1 -0.00354 0.200...
Rate of reaction Rate law Rate constant Answer Bank always has units of amount per time (i.e., molarity per second, M/s, or molarity per minute, M/min) a formula that relates reactant concentration to reaction rate can have different units, such as molarity per second (M/s), inverse seconds (s), or inverse molarity-seconds (M-.-'), depending on the reaction order symbolized as k
The differential rate law for a reaction is rate = k [A] [B]. If the rate of reaction is 0.000730 and the concentrations are [A] = 0.847 M and [B] = 0.874 M, what is the value of the rate constant? Select one: a. 0.00113 b. 8.89e-4 C. 0.00116 d. 9.86e-4 e. 7.53e-4
1)The rate law of a reaction is rate =k[X]³. The units of the rate constant areL mol-1 s-1mol² L-2 s-1mol L-1S-2L² mol-2 s-1mol L-1S-12)Given the following rate law, how does the rate of reaction change if the concentration of Z is tripled? Rate =k[X]³[Y]²[Z]⁰The rate of reaction will increase by a factor of136803)What data should be plotted to show that experimental concentration data fits a first-order reaction?1 / [reactant] vs. time[reactant] vs. timeln (k) vs. Ealn (k) vs. 1 / Tln [...