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Juliette [100K]
3 years ago
10

The pressure atop the world’s highest mountain, Mount Everest, is usually about 33.6 kPa. Convert the pressure to atmospheres. H

ow does the pressure compare with the pressure at sea level?
Chemistry
1 answer:
melomori [17]3 years ago
5 0

Answer: 0.33 atm

The pressure at Mount Everest is less as compared to pressure at seal level.

Explanation:

Pressure of the gas is defined as the force exerted by the particles on the walls of the container. It is expressed in various terms like 'mmHg', 'atm', 'kiloPascals' etc..

All these units of pressure are inter convertible.

We are given:

Pressure atop the world’s highest mountain, Mount Everest = 33.6 kPa mmHg

Converting this unit of pressure into 'atm' by using conversion factor:

1kPa= 0.0099 atm

33.6kPa=\frac{0.0099}{1}\times 33.6=0.33atm

Thus the pressure atop the world’s highest mountain, Mount Everest, is 0.33 atm

Standard sea-level pressure is 1 atmosphere.

Thus 0.33 atm at Mount Everest is less than 1 atm at sea level.

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The concentrations of the products at equilibrium are [pcl3] = 0.180 m and [cl2] = 0.250 m. what is the concentration of the rea
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We have Kc = 4.2 x 10^-2 (given but missing in the question)
and When the balanced equation for this reaction is:
PCl5(g) ↔ PCl3(g) + Cl2(g)
so, according to the Kc formula:
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so, to get the concentration of the reactants in equilibrium, the concentration of the products / the concentration of the reactants should equal the Kc value which is given in the question (missing in your question).
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Kc   = [PCl3]*[Cl2] / [PCl5]
4.2 x 10^-2 =  0.18 * 0.25 /[PCl5]
∴[PCl5] = 0.18*0.25 / 4.2x10^-2 = 1.07
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