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Imagine that you have 1.25mol of an unknown gas. It occupies a space of a quarter of a liter. If you were to add a half of a mole of gas into the container, what would the new volume of the gas be? Make the assumption that the pressure and temperature of gas remain constant. Show your work.

Answer 1

Answer:311

∘

C

Step-by-step explanation:

The idea here is that the volume and the temperature of a gas have a direct relationship when the pressure and the number of moles of gas are being kept constant

→

this is known as Charles' Law.

A very important thing to remember is that the temperature of the gas must be expressed in Kelvin. In other words, you must always work with the absolute temperature of a gas.

So, start by converting the temperature of the gas to Kelvin by using

T

[

K

]

=

t

[

∘

C

]

+

273.15

−−−−−−−−−−−−−−−−−−−−

You will have

T

=

166

∘

C

+

273.15

=

439.15 K

The volume of the gas will increase as temperature increases and decrease as temperature decreases. Mathematically, this can be written as

V

1

T

1

=

V

2

T

2

−−−−−−−−−

Here

V

1

and

T

1

represent the volume and the temperature of the gas at an initial state

V

2

and

T

2

represent the volume and the temperature of the gas at a final state

Rearrange the equation to solve for

T

2

V

1

T

1

=

V

2

T

2

⇒

T

2

=

V

2

V

1

⋅

T

1

Plug in your values to find

T

2

=

913

mL

686

mL

⋅

439.15 K

=

584.47 K

Finally, convert this to degrees Celsius

t

[

∘

C

]

=

584.47 K

−

273.15

=

311

∘

C

−−−−−−−−−−−−−−−−−−−−−−−−−−−−−−−

The answer is rounded to three sig figs.

Step-by-step explanation: