A reaction 2 A + B + 3 C → D + 5E has an initial...
A reaction 2 A + B + 3 C → D + 5E has an initial rate of 0.501 M/s and a rate law of rate = k[A][B]3[C]1/2.
What will be the initial rate if [C] is quadrupled while all other values are kept the same?
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The reaction A + B -> C + D has been found to obey the following...
The reaction A + B -> C + D has been found to obey the following rate law: rate=k[A][B]2 and has an initial rate of 0.0130 M/s. What will be the rate of the reaction if [A] is tripled and [B] is halved?
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants....
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...
Part A: For the reaction 2 A + B → C, the initial rate is measured...
Part A: For the reaction 2 A + B → C, the initial rate is measured at several different reactant concentrations. From the resulting tabulated data, determine the rate constant for the reaction. [A](M) [B](M) Initial Rate (M/s) 0.05 0.05 0.035 0.10 0.05 0.070 0.20 0.10 0.28 Answers?: 1.4×102M−2⋅s−1, 2.8×102M−2⋅s−1, 28M−2⋅s−1, 14M−1⋅s−1 Which one of these is it, and how? Part B: The aquation of tris(1,10-phenanthroline)iron(II) in acid solution takes place according to the equation: Fe(phen)32+ + 3 H3O+ +...
answer all The reaction A+B +C+D rate = k[A] [B]? has an initial rate of 0.0730...
answer all
The reaction A+B +C+D rate = k[A] [B]? has an initial rate of 0.0730 M/s. What will the initial rate be if [A] is halved and (B) is tripled? initial rate: 0.3163 M What will the initial rate be if (A] is tripled and (B) is halved? initial rate: 0.0937 For the reaction 2 H2O(g) = 2H2(g) + O2(g) the equilibrium concentrations were found to be [H,O] = 0.250 M, [H] = 0.330 M, and (0,] = 0.800...
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants....
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...
The reaction A+B rightarrow C+D rate=k[A][B]^2 has an initial rate of 0.0300 M/s. What will the...
The reaction A+B rightarrow C+D rate=k[A][B]^2 has an initial rate of 0.0300 M/s. What will the initial rate be if [A] is halved and [B] is tripled? What will the initial rate be if [A] is tripled and [B] is halved?
Question 1 2 pts Attempt due: Mar 21 Minutes, 3 Consider the below reaction: A+B -->C+D...
Question 1 2 pts Attempt due: Mar 21 Minutes, 3 Consider the below reaction: A+B -->C+D Experimental evidence indicates that the reaction proceeds according to the below mechanism: 2A --> C+E (slow) B+E -->D+A (fast) Which represents the rate law of this reaction? Rate = k[A]2 Rate = k[A][B] Rate = k*2A Rate = K[B][E] Rate = k[A] Question 2 2 pts Which integrated rate law would you utilize based on your rate law in question 1? 1/[A]t = kt...
2.c and 2.d 2. The rate law for the reaction A+B a. Write the rate law...
2.c
and 2.d
2. The rate law for the reaction A+B a. Write the rate law expression. C + D is first order in [A] and second order in [B]. Rate low- k[A] [B]² b. What is the overall order of reaction? 1 +2= 3 c. How does the rate change if [A] is halved and [B] is tripled?! d. Given the data below, propose initial concentrations for A and B that would enable you to empirically determine the given...
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants....
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
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants....
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?
answer all
The reaction A+B +C+D rate = k[A] [B]? has an initial rate of 0.0730 M/s. What will the initial rate be if [A] is halved and (B) is tripled? initial rate: 0.3163 M What will the initial rate be if (A] is tripled and (B) is halved? initial rate: 0.0937 For the reaction 2 H2O(g) = 2H2(g) + O2(g) the equilibrium concentrations were found to be [H,O] = 0.250 M, [H] = 0.330 M, and (0,] = 0.800...
The reaction A+B rightarrow C+D rate=k[A][B]^2 has an initial rate of 0.0300 M/s. What will the initial rate be if [A] is halved and [B] is tripled? What will the initial rate be if [A] is tripled and [B] is halved?
Question 1 2 pts Attempt due: Mar 21 Minutes, 3 Consider the below reaction: A+B -->C+D Experimental evidence indicates that the reaction proceeds according to the below mechanism: 2A --> C+E (slow) B+E -->D+A (fast) Which represents the rate law of this reaction? Rate = k[A]2 Rate = k[A][B] Rate = k*2A Rate = K[B][E] Rate = k[A] Question 2 2 pts Which integrated rate law would you utilize based on your rate law in question 1? 1/[A]t = kt...
2.c
and 2.d
2. The rate law for the reaction A+B a. Write the rate law expression. C + D is first order in [A] and second order in [B]. Rate low- k[A] [B]² b. What is the overall order of reaction? 1 +2= 3 c. How does the rate change if [A] is halved and [B] is tripled?! d. Given the data below, propose initial concentrations for A and B that would enable you to empirically determine the given...
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