Question

Consider the single‑step, bimolecular reaction. CH3Br+NaOH⟶CH3OH+NaBrCH3Br+NaOH⟶CH3OH+NaBr When the concentrations of CH3BrCH3Br and NaOHNaOH are both 0.140...

Consider the single‑step, bimolecular reaction.

CH3Br+NaOH⟶CH3OH+NaBrCH3Br+NaOH⟶CH3OH+NaBr

When the concentrations of CH3BrCH3Br and NaOHNaOH are both 0.140 M,0.140 M, the rate of the reaction is 0.0070 M/s.0.0070 M/s.

What is the rate of the reaction if the concentration of CH3BrCH3Br is doubled?

rate:

M/sM/s

What is the rate of the reaction if the concentration of NaOHNaOH is halved?

rate:

M/sM/s

What is the rate of the reaction if the concentrations of CH3BrCH3Br and NaOHNaOH are both increased by a factor of 3?3?

rate:

M/s

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The follwoing reaction is a single-step, bimolecular reaction: CH3Br+ NaOH -> CH3OH+NaBr When the concentrations of...
The follwoing reaction is a single-step, bimolecular reaction: CH3Br+ NaOH -> CH3OH+NaBr When the concentrations of CH3Br and NaOH are both 0.145M, the rate of the reation is 0.0020 M/s/. A) what is the rate of the reaction if the concentration of CH3Br is doubled? B) what is the rate of the reaction if the concdntration of NaOH is halved? C) what is the rate of the reaction if the concentraions of CH3Br and NaOH are both increased by a...
The following is a multi-step reaction. The rate-limiting step is unimolecular, with A as the sole...
The following is a multi-step reaction. The rate-limiting step is unimolecular, with A as the sole reactant. A+B=C+D If A and B are both .125 M, then the rate of the reaction is .0090M/s. a) What is the rate of the reaction if A is doubled? b) Starting with the original concentrations, what is the rate of the reaction if B is halved? c) Starting with the original concentrations, what is the rate of the reaction is A and B...
The following is a multi-step reaction. The rate-limiting step is unimolecular, with A as the sole...
The following is a multi-step reaction. The rate-limiting step is unimolecular, with A as the sole reactant .If [A] and [B] are both 0.195 M, then the rate of reaction is 0.0050 M/s. (a) What is the rate of the reaction if [A] is doubled (b) Starting with the original concentrations, what is the rate of the reaction if [B] is doubled? (c) Starting with the original concentrations, what is the rate of the reaction if [A] and [B] are...
Bromomethane is converted to methanol in an alkaline solution. The reaction is first order in each...
Bromomethane is converted to methanol in an alkaline solution. The reaction is first order in each reactant. CH3BR(aq)+OH-(aq)=CH3OH(aq)+Br-(aq) Write the rate law. What is the overall order of the reaction? How does the reaction rate change if the OH- concentration is decreased by a factor of 5? What is the change in rate if the concentrations of both reactants are doubled?
A mechanism for a naturally occurring reaction that destroys ozone is: Step 1: O3(g) + HO(g)...
A mechanism for a naturally occurring reaction that destroys ozone is: Step 1: O3(g) + HO(g) → HO2(g) + O2(g) Step 2: HO2(g) + O(g) → HO(g) + O2(g) Which species is a catalyst and what type of catalysis is occurring? Select one: A. HO, heterogeneous B. HO2, heterogeneous C. HO2, homogeneous D. HO, homogeneous The relative initial rates of the reaction A2 + B2 → products in vessels (a)-(d) are 1:1:4:4. Unshaded spheres represent A2 molecules, and shaded spheres...
Calculating equilibrium concentrations when the net reaction proceeds forward Consider mixture B, which will cause the...
Calculating equilibrium concentrations when the net reaction proceeds forward Consider mixture B, which will cause the net reaction to proceed forward. Concentration (M)initial:change:equilibrium:[XY]0.500−x0.500−xnet→⇌[X]0.100+x0.100+x+[Y]0.100+x0.100+x The change in concentration, x, is negative for the reactants because they are consumed and positive for the products because they are produced. Part B Based on a Kc value of 0.130 and the given data table, what are the equilibrium concentrations of XY, X, and Y, respectively? Express the molar concentrations numerically. Calculating equilibrium concentrations when...
Consider the following data showing the initial rate of a reaction (A→products) at several different concentrations...
Consider the following data showing the initial rate of a reaction (A→products) at several different concentrations of A. [A](M) Initial Rate (M/s) 0.15 6.87×10−3 0.30 1.37×10−2 0.60 2.75×10−2 What is the rate law for this reaction? Rate = k[A]3 Rate = k[A] Rate = k Rate = k[A]2 2.) Consider the following data showing the initial rate of a reaction (A→products) at several different concentrations of A. [A](M) Initial Rate (M/s) 0.15 2.75×10−2 0.30 2.75×10−2 0.60 2.75×10−2 What is the...
Learning Goal: To understand reaction order and rate constants. For the general equation aA+bB?cC+dD, the rate...
Learning Goal: To understand reaction order and rate constants. For the general equation aA+bB?cC+dD, the rate law is expressed as follows: rate=k[A]m[B]n where m and n indicate the order of the reaction with respect to each reactant and must be determined experimentally and k is the rate constant, which is specific to each reaction. Order For a particular reaction, aA+bB+cC?dD, the rate law was experimentally determined to be rate=k[A]0[B]1[C]2=k[B][C]2 This equation is zero order with respect to A. Therefore, changing...
1. Given the reaction 2A + 3B à C + 4D the reaction is zeroth order...
1. Given the reaction 2A + 3B à C + 4D the reaction is zeroth order with respect to A and second order with respect to B. If the concentration of both A and B are doubled and the temperature remains unchanged, the rate of the reaction will increase by a factor of what?   Why? 2.      The kinetics of the reaction A+B à P were studied. The following data was collected. What is the rate law for this reaction?   Why?...
11. You and your lab partner are studying the rate of a reaction, A + B...
11. You and your lab partner are studying the rate of a reaction, A + B --> C. You make measurements of the initial rate under the following conditions: Experiment [A] (M) [B] (M) Rate (M/s) 1 0.7    1.6 2 1.4 1.6 (a) Which of the following reactant concentrations could you use for experiment 3 in order to determine the rate law, assuming that the rate law is of the form, Rate = k [A]x [B]y? Choose all correct...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT