Balanced equation for the reaction of iodide ion with hypochlorite ion

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Answer 1

Question

Chapter 13, Problem 13.130CP

(a)

Interpretation Introduction

To Write:

Balanced equation for the reaction of iodide ion with hypochlorite ion

b)

Interpretation Introduction

To determine:

The rate law and Rate constant for all 4 experiments

Interpretation Introduction

To find the rate Constant: (for I^-& OCl^-)

k=2.30310log2.40×10−42.17×10−4=1.0×10−2

k=2.30310log1.60×10−41.37×10−4=1.5×10−2

Experiment − 2: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 1.20 ( 10-4 , Final conc. = 1.08 ( 10-4 & 1.60 ( 10-4 , 1.48 ( 10-4

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log1.20×10−41.08×10−4=1.0×10−2

k=2.30310log1.60×10−41.48×10−4=7.7×10−3

Experiment − 3: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 2.40 ( 10-4 , Final conc. = 2.34 ( 10-4 & 4.00 ( 10-5 , 3.40 ( 10-5

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log2.40×10−42.34×10−4=2.5×10−3

k=2.30310log4.00×10−53.40×10−5=1.6×10−2

Experiment − 4: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 1.20 ( 10-4 , Final conc. = 1.14 ( 10-4 & 1.60 ( 10-4 , 1.54 ( 10-4

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log1.20×10−41.14×10−4=5.1×10−3

k=2.30310log1.60×10−41.54×10−4=3.8×10−3

Interpretation Introduction

(c)

To verify:

If the reaction occurs by a single step mechanism

(d)

Interpretation Introduction

To determine:

A mechanism that is consistent with the rate law, and express the rate constant in terms of the rate constants for the elementary steps in the mechanism

Expert Solution & Answer

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Answer 2

Question

Chapter 13, Problem 13.130CP

(a)

Interpretation Introduction

To Write:

Balanced equation for the reaction of iodide ion with hypochlorite ion

b)

Interpretation Introduction

To determine:

The rate law and Rate constant for all 4 experiments

Interpretation Introduction

To find the rate Constant: (for I^-& OCl^-)

k=2.30310log2.40×10−42.17×10−4=1.0×10−2

k=2.30310log1.60×10−41.37×10−4=1.5×10−2

Experiment − 2: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 1.20 ( 10-4 , Final conc. = 1.08 ( 10-4 & 1.60 ( 10-4 , 1.48 ( 10-4

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log1.20×10−41.08×10−4=1.0×10−2

k=2.30310log1.60×10−41.48×10−4=7.7×10−3

Experiment − 3: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 2.40 ( 10-4 , Final conc. = 2.34 ( 10-4 & 4.00 ( 10-5 , 3.40 ( 10-5

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log2.40×10−42.34×10−4=2.5×10−3

k=2.30310log4.00×10−53.40×10−5=1.6×10−2

Experiment − 4: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 1.20 ( 10-4 , Final conc. = 1.14 ( 10-4 & 1.60 ( 10-4 , 1.54 ( 10-4

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log1.20×10−41.14×10−4=5.1×10−3

k=2.30310log1.60×10−41.54×10−4=3.8×10−3

Interpretation Introduction

(c)

To verify:

If the reaction occurs by a single step mechanism

(d)

Interpretation Introduction

To determine:

A mechanism that is consistent with the rate law, and express the rate constant in terms of the rate constants for the elementary steps in the mechanism

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 13, Problem 13.130CP

(a)

Interpretation Introduction

To Write:

Balanced equation for the reaction of iodide ion with hypochlorite ion

b)

Interpretation Introduction

To determine:

The rate law and Rate constant for all 4 experiments

Interpretation Introduction

To find the rate Constant: (for I^-& OCl^-)

k=2.30310log2.40×10−42.17×10−4=1.0×10−2

k=2.30310log1.60×10−41.37×10−4=1.5×10−2

Experiment − 2: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 1.20 ( 10-4 , Final conc. = 1.08 ( 10-4 & 1.60 ( 10-4 , 1.48 ( 10-4

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log1.20×10−41.08×10−4=1.0×10−2

k=2.30310log1.60×10−41.48×10−4=7.7×10−3

Experiment − 3: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 2.40 ( 10-4 , Final conc. = 2.34 ( 10-4 & 4.00 ( 10-5 , 3.40 ( 10-5

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log2.40×10−42.34×10−4=2.5×10−3

k=2.30310log4.00×10−53.40×10−5=1.6×10−2

Experiment − 4: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 1.20 ( 10-4 , Final conc. = 1.14 ( 10-4 & 1.60 ( 10-4 , 1.54 ( 10-4

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log1.20×10−41.14×10−4=5.1×10−3

k=2.30310log1.60×10−41.54×10−4=3.8×10−3

Interpretation Introduction

(c)

To verify:

If the reaction occurs by a single step mechanism

(d)

Interpretation Introduction

To determine:

A mechanism that is consistent with the rate law, and express the rate constant in terms of the rate constants for the elementary steps in the mechanism

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 13, Problem 13.130CP

(a)

Interpretation Introduction

To Write:

Balanced equation for the reaction of iodide ion with hypochlorite ion

b)

Interpretation Introduction

To determine:

The rate law and Rate constant for all 4 experiments

Interpretation Introduction

To find the rate Constant: (for I^-& OCl^-)

k=2.30310log2.40×10−42.17×10−4=1.0×10−2

k=2.30310log1.60×10−41.37×10−4=1.5×10−2

Experiment − 2: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 1.20 ( 10-4 , Final conc. = 1.08 ( 10-4 & 1.60 ( 10-4 , 1.48 ( 10-4

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log1.20×10−41.08×10−4=1.0×10−2

k=2.30310log1.60×10−41.48×10−4=7.7×10−3

Experiment − 3: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 2.40 ( 10-4 , Final conc. = 2.34 ( 10-4 & 4.00 ( 10-5 , 3.40 ( 10-5

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log2.40×10−42.34×10−4=2.5×10−3

k=2.30310log4.00×10−53.40×10−5=1.6×10−2

Experiment − 4: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 1.20 ( 10-4 , Final conc. = 1.14 ( 10-4 & 1.60 ( 10-4 , 1.54 ( 10-4

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log1.20×10−41.14×10−4=5.1×10−3

k=2.30310log1.60×10−41.54×10−4=3.8×10−3

Interpretation Introduction

(c)

To verify:

If the reaction occurs by a single step mechanism

(d)

Interpretation Introduction

To determine:

A mechanism that is consistent with the rate law, and express the rate constant in terms of the rate constants for the elementary steps in the mechanism

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 13, Problem 13.130CP

(a)

Interpretation Introduction

To Write:

Balanced equation for the reaction of iodide ion with hypochlorite ion

b)

Interpretation Introduction

To determine:

The rate law and Rate constant for all 4 experiments

Interpretation Introduction

To find the rate Constant: (for I^-& OCl^-)

k=2.30310log2.40×10−42.17×10−4=1.0×10−2

k=2.30310log1.60×10−41.37×10−4=1.5×10−2

Experiment − 2: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 1.20 ( 10-4 , Final conc. = 1.08 ( 10-4 & 1.60 ( 10-4 , 1.48 ( 10-4

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log1.20×10−41.08×10−4=1.0×10−2

k=2.30310log1.60×10−41.48×10−4=7.7×10−3

Experiment − 3: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 2.40 ( 10-4 , Final conc. = 2.34 ( 10-4 & 4.00 ( 10-5 , 3.40 ( 10-5

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log2.40×10−42.34×10−4=2.5×10−3

k=2.30310log4.00×10−53.40×10−5=1.6×10−2

Experiment − 4: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 1.20 ( 10-4 , Final conc. = 1.14 ( 10-4 & 1.60 ( 10-4 , 1.54 ( 10-4

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log1.20×10−41.14×10−4=5.1×10−3

k=2.30310log1.60×10−41.54×10−4=3.8×10−3

Interpretation Introduction

(c)

To verify:

If the reaction occurs by a single step mechanism

(d)

Interpretation Introduction

To determine:

A mechanism that is consistent with the rate law, and express the rate constant in terms of the rate constants for the elementary steps in the mechanism

Answer 6

Chapter 13, Problem 13.130CP

(a)

Interpretation Introduction

To Write:

Balanced equation for the reaction of iodide ion with hypochlorite ion

Answer 7

Chapter 13, Problem 13.130CP

(a)

Interpretation Introduction

To Write:

Balanced equation for the reaction of iodide ion with hypochlorite ion

Answer 8

b)

Interpretation Introduction

To determine:

The rate law and Rate constant for all 4 experiments

Answer 9

b)

Interpretation Introduction

To determine:

The rate law and Rate constant for all 4 experiments

Answer 10

Interpretation Introduction

To find the rate Constant: (for I^-& OCl^-)

k=2.30310log2.40×10−42.17×10−4=1.0×10−2

k=2.30310log1.60×10−41.37×10−4=1.5×10−2

Experiment − 2: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 1.20 ( 10-4 , Final conc. = 1.08 ( 10-4 & 1.60 ( 10-4 , 1.48 ( 10-4

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log1.20×10−41.08×10−4=1.0×10−2

k=2.30310log1.60×10−41.48×10−4=7.7×10−3

Experiment − 3: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 2.40 ( 10-4 , Final conc. = 2.34 ( 10-4 & 4.00 ( 10-5 , 3.40 ( 10-5

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log2.40×10−42.34×10−4=2.5×10−3

k=2.30310log4.00×10−53.40×10−5=1.6×10−2

Experiment − 4: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 1.20 ( 10-4 , Final conc. = 1.14 ( 10-4 & 1.60 ( 10-4 , 1.54 ( 10-4

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log1.20×10−41.14×10−4=5.1×10−3

k=2.30310log1.60×10−41.54×10−4=3.8×10−3

Answer 11

Interpretation Introduction

To find the rate Constant: (for I^-& OCl^-)

k=2.30310log2.40×10−42.17×10−4=1.0×10−2

k=2.30310log1.60×10−41.37×10−4=1.5×10−2

Experiment − 2: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 1.20 ( 10-4 , Final conc. = 1.08 ( 10-4 & 1.60 ( 10-4 , 1.48 ( 10-4

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log1.20×10−41.08×10−4=1.0×10−2

k=2.30310log1.60×10−41.48×10−4=7.7×10−3

Experiment − 3: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 2.40 ( 10-4 , Final conc. = 2.34 ( 10-4 & 4.00 ( 10-5 , 3.40 ( 10-5

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log2.40×10−42.34×10−4=2.5×10−3

k=2.30310log4.00×10−53.40×10−5=1.6×10−2

Experiment − 4: (for I^-& OCl^-)

Given Data:

Initial time = 0 &Final time = 10s
Initial conc. = 1.20 ( 10-4 , Final conc. = 1.14 ( 10-4 & 1.60 ( 10-4 , 1.54 ( 10-4

Formula Used:k=2.303tlog[I−]0[I−]10

k=2.303tlog[OCl−]0[OCl−]10

Calculation to find the rate Constants:
k=2.30310log1.20×10−41.14×10−4=5.1×10−3

k=2.30310log1.60×10−41.54×10−4=3.8×10−3

Answer 12

Interpretation Introduction

(c)

To verify:

If the reaction occurs by a single step mechanism

Answer 13

Interpretation Introduction

(c)

To verify:

If the reaction occurs by a single step mechanism

Answer 14

(d)

Interpretation Introduction

To determine:

A mechanism that is consistent with the rate law, and express the rate constant in terms of the rate constants for the elementary steps in the mechanism

Answer 15

(d)

Interpretation Introduction

To determine:

A mechanism that is consistent with the rate law, and express the rate constant in terms of the rate constants for the elementary steps in the mechanism

Answer 16

Expert Solution & Answer

Answer 17

Expert Solution & Answer

Answer 18

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Check out a sample textbook solution

See solution

Answer 19

Ch. 13 - Prob. 13.1P Ch. 13 - Prob. 13.2A Ch. 13 - Prob. 13.3P Ch. 13 - Prob. 13.4A Ch. 13 - Prob. 13.5P Ch. 13 - Prob. 13.6A Ch. 13 - Prob. 13.7P Ch. 13 - Prob. 13.8A Ch. 13 - Prob. 13.9P Ch. 13 - Prob. 13.10A

Balanced equation for the reaction of iodide ion with hypochlorite ion

To Write: Balanced equation for the reaction of iodide ion with hypochlorite ion

To determine: The rate law and Rate constant for all 4 experiments

(c) To verify: If the reaction occurs by a single step mechanism

To determine: A mechanism that is consistent with the rate law, and express the rate constant in terms of the rate constants for the elementary steps in the mechanism

Want to see the full answer?

Chapter 13 Solutions

To Write:

Balanced equation for the reaction of iodide ion with hypochlorite ion

To determine:

The rate law and Rate constant for all 4 experiments

(c)

To verify:

If the reaction occurs by a single step mechanism

To determine:

A mechanism that is consistent with the rate law, and express the rate constant in terms of the rate constants for the elementary steps in the mechanism