If the rate law for the clock reaction is: Rate = k [ I-] [ BrO3...

If the rate law for the clock reaction is: Rate = k [ I-] [ BrO3 -] [H+] A clock reaction is run with the following initial concentrations: [I-] [BrO3-] [H+] [S2O32-] 0.002 0.008 0.02 0.0001 The reaction time is 28 seconds Calculate k in the rate law:

Also:

Rate = k [ I-] [ BrO3 -] [H+] A clock reaction is run at 19 ºC with the following initial concentrations [I-] [BrO3-] [H+] [S2O32-] 0.002 0.008 0.02 0.0001 Then the experiment is repeated at 33 ºC, the rate constant k is found to be 2.7 times larger. Calculate the activation energy

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

The rate law for the reaction below is given by Rate = k(P ). At 680°C,...

The rate law for the reaction below is given by Rate = k(P ). At 680°C, the half-life is 35.0 s. Given initial pressures of P = 0.67 atm, P = 0.75 atm, and P = 0.25 atm, how many seconds will it take for the pressure of PH to drop to 0.50 atm 4 PH (g) → P (g) + 6 H (g)

1. Assume that the rate law for a reaction is rate = k[A][B]^2 a) what is...

1. Assume that the rate law for a reaction is rate = k[A][B]^2 a) what is the overall order of the reaction? b) if the concentration of both A and B are doubled, how will this affect the rate of the reaction? c) how will doubling the concentration of A, while the concentration of B is kept constant, affect the value of k (assume that temperature does not change)? how is the rate affected? 2. It is found for the...

1. The rate law for a given reaction is rate = k[NOBr]2. The rate constant is...

1. The rate law for a given reaction is rate = k[NOBr]2. The rate constant is 1.0 x 10-5 1/M∙s, and the initial concentration was 0.100 M. What is the first half-life of this reaction? A) 0.50 s B) 6.9 x 104 s C) 1.0 x 10-5 s D) 1.0 x 106 s E) None of these 2. The reaction SO2Cl2 SO2 + Cl2 is first order in SO2Cl2. If the concentration of SO2Cl2 after 198 s is 1.47 x...

1 Still for the reaction: 3BrO-(aq) --> BrO3-(aq) + 2Br-(aq), what is the rate of reaction...

1 Still for the reaction: 3BrO-(aq) --> BrO3-(aq) + 2Br-(aq), what is the rate of reaction in M/s, if Δ[BrO- ]/Δt = -0.020 M/s? 2 Under a different set of conditions Δ[BrO3- ]/Δt = 0.019 M/s. What is the rate of reaction in M/s? 3 Under a different set of conditions Δ[Br- ]/Δt = 0.016 M/s. What is the rate of reaction in M/s? 4 If Δ[BrO3- ]/Δt = 0.021 M/s. What is Δ[Br- ]/Δt in M/s? Reminder, the rate...

difference between the rate of a reaction, the reaction rate, and the rate law

Can you explain the difference between the rate of a reaction, the reaction rate, and the rate law? Also is there a difference between average rate of concentration change and instantaneous rate of concentration change, and how do they relate to the rate law? Please explain!

The reaction 2A + B → C obeys the rate law –rB = kCB2, where k...

The reaction 2A + B → C obeys the rate law –rB = kCB2, where k = 0.25 L/mol.s at 75˚C. A is available as a 1.5 M solution and B as a 1 M solution. a) A 26 L/s stream of solution A and 30 L/s stream of solution B are combined just before being introduced into a CSTR. If a 150 L reactor is available, how many mole/h of C could be produced? b) You receive some financing...

Explain what “k” means, and how it can be calculated for the iodine clock reaction. As...

Explain what “k” means, and how it can be calculated for the iodine clock reaction. As part of your explanation, include a sample calculation. Explain in one well-developed paragraph.

For the following reaction: 2HI (g) ----> H2(g) + I2(g), the rate law is rate= k[HI]^2....

For the following reaction: 2HI (g) ----> H2(g) + I2(g), the rate law is rate= k[HI]^2. You are starting with 1.0M HI. How long will the first half-life reaction be? (The professor adds: Note that since you don't know the value for the rate constant k, just leave it in your answers.)

The reaction 2NO(g) + Cl2(g) --> 2NOCl(g) obeys the rate law rate = k [NO]2 [Cl2]....

The reaction 2NO(g) + Cl2(g) --> 2NOCl(g) obeys the rate law rate = k [NO]2 [Cl2]. The following mechanism is proposed: NO (g) + Cl2 (g) --> NOCl2(g) NOCl2(g) + NO (g) -->2NOCl (g) a) What would the rate law be if the first step was rate determining? b) Based on the observed rate law, what can be concluded about the relative rates of the 2 reactions?

) Consider the reaction A à products. The rate law for this reaction is rate =...

) Consider the reaction A à products. The rate law for this reaction is rate = k[A] where k=7.02 ´ 10-3 M-1 s-1 at a particular temperature. If the initial [A] = 0.0500 M, what is the initial rate? What is the value of the half-life for this initial concentration of A? What will be the half-life if the initial [A] = 0.0250 M What will be the half-life if the initial [A] = 0.100 M What will be the...

Subjects