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3 years ago

21.7 mL of gas at 98.8 kPa is allowed to expand at constant

Chemistry

1 answer:

IRISSAK [1]3 years ago

5 0

Answer: 40.68 kPa

Explanation:

Given that,

Original volume of gas V1 = 21.7 mL

Original pressure of gas P1 = 98.8 kPa

New volume of gas V2 = 52.7 mL

New pressure of gas P2 = ?

Since pressure and volume are given while temperature is constant, apply the formula for Boyle's law

P1V1 = P2V2

98.8 kPa x 21.7 mL = P2 x 52.7L

2143.96 kPa L = 52.7 L x P2

P2 = 2143.96 kPa L / 52.7 L

P2 = 40.68 kPa

Thus, the new pressure of the gas is 40.68 kPa.

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Hence, letter C is the correct answer.

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3 years ago

Be sure to answer all parts. Consider the following balanced redox reaction (do not include state of matter in your answers): 2C

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Answer:

The specie which is oxidized is:- $CrO_2^-$

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Explanation:

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For the given chemical reaction:

$2CrO_2^- + 6ClO^- + 2H_2O\rightarrow 2CrO_4^{2-} + 3Cl_2 + 4OH^-$

The half cell reactions for the above reaction follows:

Oxidation half reaction: $CrO_2^- + 2H_2O + 4OH^-\rightarrow CrO_4^{2-} + 4H_2O + 3e^-$

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Thus, the specie which is oxidized is:- $CrO_2^-$

The specie which is reduced is:- $ClO^-$

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4 years ago

All three of the phosphorus-fluorine single bonds in pf3 are polar. in which direction should the polarity arrows point?

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3 years ago

Why vitamin A(retinol) transported by chylomicrons ?

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Answer:

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3 years ago

A sample of oxygen gas is compressed from 30.6 L to 1.8 L at constant temperature pressure of 1.8 atm. Calculate the amount of e

ad-work [718]

Answer:

the change in the internal energy of the system is 3,752.67 J

Explanation:

Given;

initial volume of the gas, V₁ = 30.6 L

final volume of the gas, V₂ = 1.8 L

constant pressure of the gas, P = 1.8 atm

Energy released by the system, Q = 1.5 kJ = 1,500 J

Apply pressure-volume work equation, to determine the work done on the gas;

w = -PΔV

w = -P(V₂ - V₁)

w = - 1.8 atm(1.8 L - 30.6 L)

w = 51.84 L.atm

w = 51.84 L.atm x 101.325 J/L.atm

w = 5,252.67 J

The change in the internal energy of the system is calculated as;

ΔU = Q + w

Since the heat is given out, Q = - 1,500 J

ΔU = -1,500 J + 5,252.67 J

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Therefore, the change in the internal energy of the system is 3,752.67 J

3 0

3 years ago