Rate law and order (in each reactant or overall) from the orders or a given rate law

1. A.
   Overall order of reaction is 2.
2. B.
   The reaction is first order in H$_2$.
3. C.
   The reaction is first order in I$_2$.
4. D.
   Overall order of reaction is 1.

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1. A.
   $r = k[\text{NO}_2]^{1/2}[\text{CO}]$
2. B.
   $r = k[\text{NO}_2]^2[\text{CO}]^0$
3. C.
   $r = \frac{1}{2}k[\text{NO}_2][\text{CO}]$
4. D.
   $r = k[\text{NO}_2]^2[\text{CO}]$

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1. A.
   0, 2
2. B.
   1, 3
3. C.
   2, 1
4. D.
   3, 1

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1. A.
   Rate $=k[\text{NO}]^{2}[\text{Cl}_{2}]$
2. B.
   Rate $=k[\text{NO}][\text{Cl}_{2}]$
3. C.
   Rate $=k[\text{NO}]^{2}$
4. D.
   Rate $=k[\text{Cl}_{2}]$

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1. A.
   Rate $=k[\text{CHCl}_3][\text{Cl}_2]^{1/2}$
2. B.
   Rate $=k[\text{CHCl}_4]^2[\text{Cl}_2]^{1/2}$
3. C.
   Rate $=k[\text{CHCl}_3]^{3/2}[\text{Cl}_2]$
4. D.
   Rate $=k[\text{CHCl}_3]^{1/2}[\text{Cl}_2]$

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1. A.
   1.5
2. B.
   2.5
3. C.
   +1
4. D.
   4

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1. A.
   $0$
2. B.
   $1$
3. C.
   $2$
4. D.
   $3$

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