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m_a_m_a [10]
3 years ago
9

For a reaction that follows the general rate law, Rate = k[A][B]2, what will happen to the rate of reaction if the concentration

of A is increased by a factor of 5.00?4
Chemistry
1 answer:
sleet_krkn [62]3 years ago
5 0

Answer:

The rate will increase by a factor of 5.00 too.

Explanation:

Hello,

In this case, given the rate law:

r=k[A][B]^2

Thus, we can notice it is first-order respect to A, for that reason, increasing its concentration by a factor of 5.00, increase the rate by a factor of 5.00 as well.

Moreover, if the concentration of B is increased by the same factor, the rate will increase by a factor of 25.00, since the rate is second-order respect to B (it is squared).

Best regards.

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Which of these, if dissolved in 1.0 l of pure water, would produce a buffer solution? which of these, if dissolved in 1.0 l of p
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Answer:

  1. (0.1 mol NaH₂PO₄ + 0.1 mol Na₂HPO₄)

Explanation:

A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate base, or weak base and its conjugate acid.

Also, a buffer solution is a solution which resists changes in pH when acid or alkali is added to it.

  1. (0.1 mol NaH₂PO₄ + 0.1 mol Na₂HPO₄) when dissolved in 1 L H₂O will produce a buffer because NaH₂PO₄ is considered as weak acid while Na₂HPO₄ is its conjugate base. 2.
  2. (0.1 mol H₃O⁺ + 0.1 mol Cl⁻) is not a mixture of a weak acid and its conjugate base, or weak base and its conjugate acid.
  3. (0.1 mol HCl + 0.1 mol NaoH) HCL is a strong acid and NaOH is a strong base so it will not form a buffer when dissolved in water.
  4. (0.1 mol H₃O⁺ + 0.1 OH⁻) is not a mixture of a weak acid and its conjugate base, or weak base and its conjugate acid
  5. (0.1 mol NaCl+ 0.1 mol KCl) NaCL and KCL are salts so it will not form a buffer when dissolved in water.

So the right choice is

  1. (0.1 mol NaH₂PO₄ + 0.1 mol Na₂HPO₄)

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