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4 years ago

Which of these statements is not true about chemical reaction rates

Chemistry

2 answers:

grin007 [14]4 years ago

6 0

Answer: The statement (B) is not true about chemical reactions.

Explanation:

A chemical reaction rate is affected by the several factors few of which are temperature, concentration of reactants, surface area etc.

In a chemical reaction, if temperature is increased then the rate of reaction will increase because it will increase the average kinetic energy of the reactant molecules. Thus, large number of molecules will have minimum energy required for an effective collision.

It is known that increasing the amount of reactants will increase the rate of reaction.

Therefore, rate of reaction will change if concentration or temperature is changed.

Hence, the statement (B) is not true about chemical reactions.

storchak [24]4 years ago

4 0

Answer B because temperature can affect the reaction rate.

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qaws [65]

Answer:

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Explanation:

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3 years ago

Monochloroacetic acid (HC2H2ClO2) is a skin irritant that is used in "chemical peels" intended to remove the top layer of dead s

yaroslaw [1]

Answer: The pH of the solution is 1.703

Explanation:

We are given:

Concentration of monochloroacetic acid = 0.31 M

The chemical equation for the dissociation of monochloroacetic acid follows:

$HC_2H_2ClO_2\rightleftharpoons H^++C_2H_2ClO_2^-$

Initial: 0.31

At eqllm: 0.31-x x x

The expression of $K_a$ for above equation follows:

$K_a=\frac{[H^+][C_2H_2ClO_2^-}}{[HC_2H_2ClO_2]}$

We are given:

$K_a=1.35\times 10^{-3}$

Putting values in above equation follows:

$1.35\times 10^{-3}=\frac{x\times x}{(0.31-x)}\\\\x=-0.021,0.0198$

Neglecting the negative value of 'x' because concentration cannot be negative.

To calculate the pH of the solution, we use the equation:

$pH=-\log[H^+]$

$pH=-\log (0.0198)\\\\pH=1.703$

Hence, the pH of the solution is 1.703

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4 years ago

Matching

valentinak56 [21]

N to church ⛪️ for church ⛪️ church ⛪️ and

3 0

3 years ago

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