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Rainbow [258]
4 years ago
14

For the hypothetical reaction A → B, calculate the average rate of disappearance of A if the initial concentration of A is 0.91

M and the concentration of A after 90 minutes is 0.11 M.
a. 8.9 * 10^-3 M/min
b. -8.9 * 10^-3 M/min
c. 8.9 * 10^-3 M/min
d. 0.80 M/min
Chemistry
1 answer:
galben [10]4 years ago
7 0

<u>Answer:</u> The average rate of disappearance of A is 8.9\times 10^{-3}M/min

<u>Explanation:</u>

The given chemical reaction follows:

A\rightarrow B

The average rate of the reaction for disappearance of A is given as:

\text{Average rate of disappearance of A}=-\frac{\Delta [A]}{\Delta t}

Or,

\text{Average rate of disappearance of A}=-\frac{C_2-C_1}{t_2-t_1}

where,

C_2 = final concentration of A = 0.11 M

C_1 = initial concentration of A = 0.91 M

t_2 = final time = 90 minutes

t_1 = initial time = 0 minutes

Putting values in above equation, we get:

\text{Average rate of disappearance of A}=-\frac{0.11-0.91}{90}\\\\\text{Average rate of disappearance of A}=8.9\times 10^{-3}M/min

Hence, the average rate of disappearance of A is 8.9\times 10^{-3}M/min

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