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3 years ago

Consider the following three-step representation of a reaction mechanism.

Chemistry

2 answers:

suter [353]3 years ago

6 0

Answer:

The answer is C. AB is an intermediate; therefore the rate law is determined from the reactants in the previous step.

I just took the test and C. was correct. Please mark me as brainliest!

AlladinOne [14]3 years ago

6 0

Answer: C: AB is an intermediate; therefore the rate law is determined from the reactants in the previous step.

Explanation: : Rate law is usually determined from the slowest step of the reaction mechanism.

Thus as we can see that the reaction which is slow has AB as its intermediate, rate law can be determined from the same.

Moreover , we can see that the overall rate law is very different from the rat law determined from the slowest step.

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When 70.4 g of benzamide (C7H7NO) are dissolved in 850. g of a certain mystery liquid X , the freezing point of the solution is

lora16 [44]

Answer:

i=1.62 .

Explanation:

Let, i be the Van't Hoff Factor.

Moles of benzamide,= $\dfrac{Mass}{molar\ mass}=\dfrac{70.4}{121.14}=0.58\ mol.$

Molality of solution, m= $\dfrac{moles }{mass\ of\ solvent}=\dfrac{0.58}{0.85}=0.68\ molal.$

Now, we know

Depression in freezing point, $\Delta T=i\times K_f\times m$ .....1

It is given that,

$\Delta T=2.7^o C\\i=1 ( since\ it\ is\ non\ dissociable\ solutes)\\K_f ( freezing\ constant)\\$

Putting all these values we get,

$K_f=3.949\ C/m.$

Now, moles of ammonium chloride= $\dfrac{70.4}{53.49}=1.316\ mol.$

molality = $\dfrac{1.316}{0.85}=1.54 molal.\\\Delta T=9.9 .$

Putting all these values in eqn 1.

We get,

i=1.62 .

Hence, this is the required solution.

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