3. A sample of krypton gas occupies 75.0 mL at 0.400 atm. If the temperature remained constant, what volume would the krypton occupy at:

c. 765 mmHg; d. 4.00 mmHg; e. 3.50x10-2

c) 29.8 mL

d) 5375 mL

e)

Explanation:

c)

We can solve this problem by using Boyle's Law, which states that:

"For a fixed mass of an ideal gas kept at constant temperature, the pressure of the gas is inversely proportional to its volume"

Mathematically:

where

p is the pressure of the gas

V is its volume

We can rewrite the formula as

For the gas in this problem:

is the initial pressure

is the initial volume

is the final pressure (using the conversion factor )

Solving for V2, we find the final volume:

d)

We can solve this part by using again the equation:

Where in this case we have:

is the initial pressure

is the initial volume

is the final pressure

Converting into atmospheres,

And solving for V2, we find the final volume:

e)

As before, we use Boyles' Law:

In this part we have:

is the initial pressure of the gas

is the initial volume of the gas

1 torr is equivalent to 1 mmHg, so the conversion factor is the same as before, therefore the final pressure in atmospheres is:

And so, the final volume of the krypton gas is:

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