[A] M 0.200 0.200 0.400 The order in A is The order in B is k= O k=[A]²[B] Ok=[A][B]² [B] M O K=[A][B] 0.0800 0.160 0.160 rate = k[A]²[B] Using the data in Table 1, fill in the blanks with a whole number (0,1,2,3,etc) rate = k[A][B] O M²s-¹ Initial rate of production of Given the data in Table 1, what is the correct rate law for the reaction? rate = k[A][B]² C M/S 0.500 1.00 4.00 Given the value in Table 1, calculate the numerical value of k to three significant figures Given the data in Table 1, what are the units of k? O MS-1 O M-²S-1
[A] M 0.200 0.200 0.400 The order in A is The order in B is k= O k=[A]²[B] Ok=[A][B]² [B] M O K=[A][B] 0.0800 0.160 0.160 rate = k[A]²[B] Using the data in Table 1, fill in the blanks with a whole number (0,1,2,3,etc) rate = k[A][B] O M²s-¹ Initial rate of production of Given the data in Table 1, what is the correct rate law for the reaction? rate = k[A][B]² C M/S 0.500 1.00 4.00 Given the value in Table 1, calculate the numerical value of k to three significant figures Given the data in Table 1, what are the units of k? O MS-1 O M-²S-1
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter1: The Nature Of Chemistry
Section: Chapter Questions
Problem 110QRT
Related questions
Question
![Table 1
[A]
M
0.200
0.200
0.400
The order in A is
The order in B is
k=
Ok=[A]²[B]
Ok=[A][B]²
[B]
M
O k=[A][B]
0.0800
0.160
0.160
rate = k[A]²[B]
Using the data in Table 1, fill in the blanks
with a whole number (0,1,2,3,etc)
rate = k[A][B]
O
M²s-1
Initial rate of
production of
Given the data in Table 1, what is the
correct rate law for the reaction?
rate = k[A][B]²
C
M/S
0.500
1.00
4.00
Given the value in Table 1, calculate the
numerical value of k to three significant
figures
Given the data in Table 1, what are the
units of k?
O Ms¹
O M-²S-1](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F128b16fc-49af-4250-a5b9-9c298fcd5812%2F13c44a15-73c6-45a7-a13e-988708dfa237%2Fhs8mx3t_processed.png&w=3840&q=75)
Transcribed Image Text:Table 1
[A]
M
0.200
0.200
0.400
The order in A is
The order in B is
k=
Ok=[A]²[B]
Ok=[A][B]²
[B]
M
O k=[A][B]
0.0800
0.160
0.160
rate = k[A]²[B]
Using the data in Table 1, fill in the blanks
with a whole number (0,1,2,3,etc)
rate = k[A][B]
O
M²s-1
Initial rate of
production of
Given the data in Table 1, what is the
correct rate law for the reaction?
rate = k[A][B]²
C
M/S
0.500
1.00
4.00
Given the value in Table 1, calculate the
numerical value of k to three significant
figures
Given the data in Table 1, what are the
units of k?
O Ms¹
O M-²S-1
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