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# Application of Method of Initial Rates to Table Data

APCHEM-XKPKTV

The table below shows recorded concentration data for the following chemical reaction:

$$Ca{ Cl }_{ 2 }(aq)+2AgN{ O }_{ 3 }(aq) \longrightarrow Ca{ (N{ O }_{ 3 }) }_{ 2 }(aq)+2AgCl(s)$$

$$\text{rate} = k{ [Ca{ Cl }_{ 2 }] }^{ x }{ [AgN{ O }_{ 3 }] }^{ y }$$

$[CaCl_2] \ \text{M} \quad$ $[AgNO_3] \ \text{M} \quad$ $\text{Rate M/s} \quad$
$0.050$ $0.050$ $3.33 \times 10^{-3} \quad$
$0.100$ $0.050$ $6.66 \times 10^{-3}$
$0.100$ $0.100$ $13.32 \times 10^{-3} \quad$

$\$

Using the data, the exponents $x$ and $y$ in the rate law are

A

$x = 2$, $y=3$

B

$x = 1$, $y = 2$

C

$x = 1$, $y = 1$

D

$x = 2$, $y = 2$