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A gas occupies 11.2 L at a pressure of 35.0 mm . What is the volume of the gas if it is Increased to a pressure of 64.0 mm Hg?
A) 6.13 L
B) 110.2 L
C) 200.0 K
D) 20.5 L

Sagot :

Explanation:

[tex]from \: boyle's \: law \\ P _{1} V _{1} = P _{2} V _{2} \\ 35 \times 11.2 = 64 \times V _{2} \\ V _{2} = \frac{35 \times 11.2}{64} \\ V _{2} = 6.125 \: L[/tex]

The volume of the gas is 6.13 l if it is increased to a pressure of 64.0 mm Hg.

Boyle's Law

Boyle's law is a gas law which states that at constant temperature, the pressure of a given quantity of a gas varies inversely with its volume occupied by it.  

According to the Boyle's Law:

PV = constant

Thus,

[tex]P_{1}V_{1} = P_{2} V_{2}[/tex]

where,

[tex]P_{1}[/tex] is the initial pressure

[tex]V_{1}[/tex] is the initial volume

[tex]P_{2}[/tex] is the final pressure

[tex]V_{2}[/tex] is the final volume

Now, put the values in above equation we get

[tex]P_{1} V_{1} = P_{2} V_{2}[/tex]

35.0 × 11.2 = 64.0 × [tex]V_{2}[/tex]

392 = 64.0 × [tex]V_{2}[/tex]

[tex]V_{2}[/tex] = [tex]\frac{392}{64}[/tex]

[tex]V_{2}[/tex] = 6.13 L

Thus, the volume of the gas is 6.13 l if it is increased to a pressure of 64.0 mm Hg.

Learn more on about the Boyle's Law here:  https://brainly.com/question/1696010

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