The reaction
A+ B yields C+D
rate = k[A][B]^2
has an intial rate of 0.0220 M/s
what will the initial rate be if [A] is halved and [B] is tripled? answer must be in M/s
What will the intial rate be if [A] is tripled and [B] is
halved? answer must be in M/s
The concept used to solve this problem is based on rate law of a chemical reaction.
Rate law is an equation that establishes a link between the concentration of the reactants and the rate of the reaction.
For a chemical reaction,
The rate law is written as follow.
Here, is the concentration of reactant , is the concentration of reactant , is the rate constant of the reaction, and are the reaction orders which is an experimentally determined quantity.
Part 1
The reaction is:
The rate law for this reaction is written as:
Substitute initial rate of the reaction in rate law.
An expression for initial rate is obtained using the rate law by substituting the value of initial rate.
Part 1
When is halved and is tripled, the new concentrations are:
and
The new rate law is written as:
Substitute, for and for in new rate law as follows:
\u2026\u2026 (1)
Since,
Substitute, for in equation (1), thus
Rate of the reaction become .
The rate of the reaction when is halved and is tripled is .
When the initial concentrations of the reactants are changed by any factor, then the first step is to write the new concentrations in terms of the initial concentrations. Then, write the new rate law in terms of the initial concentrations. And then calculate the new rate law by substituting the values accordingly.
Part 2
When is tripled and is halved, so the new concentrations are:
and
The new rate law is written as:
Substitute, for and for in new rate law as follows:
\u2026\u2026 (2)
Since,
Substitute, for in equation (2), thus
Rate of the reaction become .
The rate of the reaction when is tripled and is halved is .
When the initial concentrations of the reactants are changed by any factor, then the first step is to write the new concentrations in terms of the initial concentrations. Then, write the new rate law in terms of the initial concentrations. And then calculate the new rate law by substituting the values accordingly.
The rate of the reaction when is halved and is tripled is .
The rate of the reaction when is tripled and is halved is .
The rate of the reaction when is halved and is tripled is .
The rate of the reaction when is tripled and is halved is .
What will the initial rate be if [A] is tripled and [B] is halved? The reaction A + B + C +D rate k[A][B]2 has an initial rate of 0.0920 M/s.
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?
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 -> 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?
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...
Consider the following reaction: A + B + C +D The rate law for this reaction is as follows: Rate = k Alla B11/2 Suppose the rate of the reaction at certain initial concentrations of A, B, and C is 1.14x10-2 M/s. Part A What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled? VO AED A O O ? Rate 2 = M/s Submit Request Answer
Review Constants Periodic Table Consider the following reaction: A + B + C D The rate law for this reaction is as follows: Part A Rate = k., A][C] B1/2 What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled? Suppose the rate of the reaction at certain initial concentrations of A, B, and C is 1.19x10-2 M/s. 18 AU A O O ? Rate 2 =...
What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled? Exercise 14.85 13 of 32 > I Review | Constants 1 Periodic Table Consider the following reaction: A + B + C + D The rate law for this reaction is as follows: Part A Rate = k[A][C] B11/2 What is the rate of the reaction if the concentrations of A and C are doubled and the...
Consider the following reaction: A+B+C→D The rate law for this reaction is as follows: Rate=k[A][C]2[B]1/2 Suppose the rate of the reaction at certain initial concentrations of A, B, and C is 1.19×10−2 mol⋅L−1⋅s−1 . What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled?
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...