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alexira [117]
3 years ago
13

The N2O4−NO2 reversible reaction is found to have the following equilibrium partial pressures at 100∘C. Calculate Kp for the rea

ction. N2O4(g)⇌2NO2(g) 0.0005 atm 0.095 atm Express your answer using two significant figures.
Chemistry
1 answer:
timofeeve [1]3 years ago
3 0

Answer:

K_{p} for the reaction is 18.05

Explanation:

Equilibrium constant in terms of partial pressure (K_{p}) for this reaction can be written as-

                K_{p}=\frac{P_{NO_{2}}^{2}}{P_{N_{2}O_{4}}}

where P_{NO_{2}} and P_{N_{2}O_{4}} are equilibrium partial pressure of NO_{2} and N_{2}O_{4} respectively

Hence K_{p}=\frac{(0.095)^{2}}{(0.0005)} = 18.05

So, K_{p} for the reaction is 18.05

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Answer:

<u>The new pressure is 1.0533 atm</u>

<u></u>

Explanation:

According  to<u> Boyle's Law :</u> The Pressure of fixed amount of gas is inversely proportional to Volume at constant temperature.

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3 years ago
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Nastasia [14]

Answer:

See explanation

Explanation:

The question is incomplete because the image of the alcohol is missing. However, I will try give you a general picture of the reaction known as hydroboration of alkenes.

This reaction occurs in two steps. In the first step, -BH2 and H add to the same face of the double bond (syn addition).

In the second step, alkaline hydrogen peroxide is added and the alcohol is formed.

Note that the BH2 and H adds to the two atoms of the double bond. The final product of the reaction appears as if water was added to the original alkene following an anti-Markovnikov mechanism.

Steric hindrance is known to play a major role in this reaction as good yield of the anti-Markovnikov like product is obtained with alkenes having one of the carbon atoms of the double bond significantly hindered.

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Answer:

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Explanation:

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