The initial rate of consumption of A in a reaction where reactants A and B produce product P was determined for various initial concentrations, with the results listed as follows: [A]0 [B]0 initial rate 1.00 M 1.00 M 0.340 M s-1 0.50 M 1.00 M 0.340 M s-1 0.25 M 0.50 M 0.085 M s-1 Which rate law is consistent with these observations
The initial rate of consumption of A in a reaction where
reactants A and B produce product P was determined for various
initial concentrations, with the results listed as
follows:
[A]0 |
[B]0 |
initial rate |
1.00 M |
1.00 M |
0.340 M s-1 |
0.50 M |
1.00 M |
0.340 M s-1 |
0.25 M |
0.50 M |
0.085 M s-1 |
Which rate law is consistent with these observations ?
The initial rate of consumption of A in a reaction where reactants A and B produce...
For the reaction A +B+C D +E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial A B C Initial rate (mol L -1 (mol L-1) (mol L -1) (mol L-'s-1) 0.50 0.50 0.50 1.5x10-4 0.50 0.50 1.50 4.5x10-4 1.00 0.50 0.50 6.0x10-4 1.00 1.00 0.50 6.0x10-4 What is the value of the rate constant k for this reaction? Express your answer to two significant figures and include the appropriate units....
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial [A] (M) [B] (M) [C] (M) Initial rate (M/s) 1 0.40 0.40 0.40 1.2×10−4 2 0.40 0.40 1.20 3.6×10−4 3 0.80 0.40 0.40 4.8×10−4 4 0.80 0.80 0.40 4.8×10−4 Rate law equation The rate of a chemical reaction depends on the concentrations of the reactants. For the general reaction between Aand B, aA+bB⇌cC+dD The dependence of the reaction...
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial [A] (M) [B] (M) [C] (M) Initial rate (M/s) 1 0.40 0.40 0.40 1.2×10−4 2 0.40 0.40 1.20 3.6×10−4 3 0.80 0.40 0.40 4.8×10−4 4 0.80 0.80 0.40 4.8×10−4 Rate law equation The rate of a chemical reaction depends on the concentrations of the reactants. For the general reaction between A and B, aA+bB⇌cC+dD The dependence of the...
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial [A] (M) [B] (M) [C] (M) Initial rate (M/s) 1 0.30 0.30 0.30 9.0×10−5 2 0.30 0.30 0.90 2.7×10−4 3 0.60 0.30 0.30 3.6×10−4 4 0.60 0.60 0.30 3.6×10−4 What is the value of the rate constant k for this reaction?
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. What is the reaction order with respect to B? Also, how do you find the value of the rate constant k for this reaction? Trial [A] (M) [B] (M) [C] (M) Initial rate (M/s) 1 0.30 0.30 0.30 9.0×10−5 2 0.30 0.30 0.90 2.7×10−4 3 0.60 0.30 0.30 3.6×10−4 4 0.60 0.60 0.30 3.6×10−4
± Experimental Determination of a Rate Law Part B: Calculate the initial rate for the formation of C at 25 ∘C, if [A]=0.50M and [B]=0.075M. Express your answer to two significant figures and include the appropriate units. Consider the reaction A+2B⇌C whose rate at 25 ∘C was measured using three different sets of initial concentrations as listed in the following table: Trial [A] (M) [B] (M) Rate (M/s) 1 0.50 0.030 9.0×10−3 2 0.50 0.060 1.8×10−2 3 1.00 0.030 3.6×10−2
For the reaction A+B+C→D+EA+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trials [A] (M) [B] (M) [C] (M) Initial rate (M/s) 1 0.20 0.20 0.20 6.0x10-5 2 0.20 0.20 0.60 1.8×10−4 3 0.40 0.20 0.20 2.4×10−4 4 0.40 0.40 0.20 2.4×10−4 Given the data calculated in Parts A, B, C, and D, determine the initial rate for a reaction that starts with 0.45 M of reagent A and 0.90 M...
(I just need part B) Consider the reaction A+2B⇌C whose rate at 25 ∘C was measured using three different sets of initial concentrations as listed in the following table: Trial [A] (M) [B] (M) Rate (M/s) 1 0.50 0.030 9.0×10−3 2 0.50 0.060 1.8×10−2 3 1.00 0.030 3.6×10−2 Part A Part complete What is the rate law for this reaction? Express the rate law symbolically in terms of k, [A], and [B]. rate = k[A]2[B] Part B Calculate the initial...
Consider the reaction A+2B⇌C whose rate at 25 ∘C was measured using three different sets of initial concentrations as listed in the following table: Trial [A] (M) [B] (M) Rate (M/s) 1 0.50 0.050 1.5×10−2 2 0.50 0.100 3.0×10−2 3 1.00 0.050 6.0×10−2 What is the rate law for this reaction? Express the rate law symbolically in terms of k, [A], and [B].
Question 23 3 pts Reaction rates at various initial concentrations of reactants were measured at 900°C for the following reaction 2NO(g) + 2H2(N) + 2 H2O() Use the data in the table to determine the rate law for the reaction. Initial Rate (M/S) Initial [NO] 0.300 0.150 0.250 Initial [H.] 0.100 0.100 0.200 5.69 x 10-2 1.42 x 10- 7.90 x 10- o Rate - k[NO] Hal o Rate - KINOJH2] o Rate -KINO Hal o Rate =kINO] [Hala Question...