Question

I NEED PART C

± Henry's Law

The solubility of a gas in a liquid increases with increasing pressure.

To understand the above statement, consider a familiar example: cola. In cola and other soft drinks, carbon dioxide gas remains dissolved in solution as long as the can or bottle remains pressurized. As soon as the lid is opened and pressure is released, the CO2 gas is much less soluble and escapes into the air.

The relationship between pressure and the solubility of a gas is expressed by Henry's law: S=kP, where S is concentration in M, k is the Henry's law constant in units of mol/(L⋠atm), and P is the pressure in atm.

Note: Since temperature also affects the solubility of a gas in an liquid, the Henry's law constant is specific to a particular gas at a particular temperature.

The following table provides some information on carbon dioxide solubility in water.

S (mol/L)	P (atm)	k (mol⋠L−1⋠atm−1)	T (∘C)
3.80×10−2	1.00		20.0
7.30×10−2			20.0
	1.00	3.40×10−2	25.0

Part A

What is the Henry's law constant for CO2 at 20∘C?

Express your answer to three significant figures and include the appropriate units.

0.0380 molL⋠atm

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Correct

Part B

What pressure is required to achieve a CO2 concentration of 7.30×10^−2 M at 20∘C?

Express your answer to three significant figures and include the appropriate units.

1.92 atm

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Correct

Part C

At 1 atm, how many moles of CO2 are released by raising the temperature of 1 liter of water from 20∘C to 25∘C?

Express your answer to four decimal places and include the appropriate units.

0.003mol

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