3 years ago

I need help with these two if you zoom in it’s clearer

Chemistry

1 answer:

makvit [3.9K]3 years ago

3 0

Answer:

It looks alittle dark can you fix it?

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The reaction described by the equation CH 3 Cl + NaOH → CH 3 OH + NaCl follows the second-order rate law, rate = k [ CH 3 Cl ] [

fredd [130]

Answer:

The rate is $4,5 \times 10^{-5}\frac{mole}{Ls}$

Explanation:

Stoichiometry

$CH_{3}Cl+NaOH \rightarrow CH_{3}OH+NaCl$

Kinetics

$-r_{A}=k \times [CH_{3}Cl] \times [NaOH]$

The rate constant K can be calculated by replacing with the initial data

$1 \times 10^{-4}\frac{mole}{Ls}=k \times [0,2M] \times [1,0M] =5 \times 10^{-4}\frac{L}{mole s}$

Taking as a base of calculus 1L, when half of the $CH_{3}Cl$ is consumed the mixture is composed by

$0,1 mole CH_{3}Cl$ (half is consumed)

$0,9 mole NaOH$ (by stoicheometry)

$0,1 mole CH_{3}OH$

$0,1 mole NaCl$

Then, the rate is

$-r_{A}=5 \times 10^{-4} \frac{L}{mole s}\times 0,1M \times 0,9 M=4,5 \times 10^{-5}\frac{mole}{Ls}$

The reaction rate decreases because there’s a smaller concentration of reactives.

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indentify one element that will combine with phosphorus in the same ratio of atoms as the ratio in aluminum phosphide

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The answer is <span>ReGallium or Indium</span>

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4 years ago

What would be the effect on this reaction of increasing the temperature?

RideAnS [48]

the correct answer to this question is C

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An excess of NiCO3, 12 g, was added to 40cm cube of sulpheric acid, 2.0 mol/dm cube. The unreacted nickel carbonate was filtered

Zepler [3.9K]

Calculate the number of moles reacted - 0.08 moles
Calculate the mass of nickel carbonate reacted - 0.08 * 119g
Calculate the mass of unreacted nickel carbonate - 12.0 - (0.08 * 119)g

1 mole of NiCO3 reacts with 1 mole of H2SO4

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3 years ago