Question

A gas that exerts a pressure of
215 torr in a container with a volume of
51.0 mL will exert a pressure of
torr when transferred to a
container with a volume of 18.5 mL.
Assume that the number of moles and the
temperature remain constant.

Answer 1

Step-by-step explanation:

According to Boyle's Law :

$p _1v _1 = p _2v _2$

$v _2 = \frac{p _1v _1}{p _2} = \frac{215 \times 51}{18.5} = 592.7ml$

Answer 2

The pressure exert in a container is 592.70 torr.

To find The pressure exert in a container.

What is Molarity?

Molarity is defined as the moles of a solute per liters of a solution. Molarity is also known as the molar concentration of a solution.

Given that :

pressure($P_{1}$)=215 torr

volume ($v_{1}$)=51.0 mL

volume($v_{2}$)= 18.5 mL

$P_{2}$=?

Number of moles and the temperature remain constant.

By the use of "Boyle's law" :

$P_{1} V_{1} =P_{2} V_{2} \\\\215*51=P_{2} *18.5\\\\P_{2} =\frac{215*51}{18.5} \\\\P_{2} =592.70 torr$

So, the pressure exert in a container is 592.70 torr.

Learn more about Molarity here:

https://brainly.com/question/17211189

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