Question

Hey sample of helium occupies 235 mL at 788 tour and 25°C. If the sample is condensed into a 0.115 L flask what will be the new pressure assuming constant temperature?

Answer 1

the system is in constant temperature

so it follows Boyle's law

i.e.P1V1=P2P2

where P1=initial pressure=788 tour

P2=final pressure= ?

V1=initial volume=235 ml

V2=final volume=0.115 ml

Answer 2

The new pressure of helium gas assuming constant temperature is equal to 1610.26 Torr.

Given the following data:

• Initial volume = 235 mL

• Final volume = 0.115 L

• Initial pressure = 788 Torr

• Temperature = 25°C.

Conversion:

Initial volume = 235 mL to L = $\frac{235}{1000} = 0.235\;L$

To determine the new pressure assuming constant temperature, we would apply Boyle's law:

Mathematically, Boyle's law is given by the formula;

$PV = k\\\\P_1V_1 = P_2V_2$

Where;

• $P_1$ is the original (initial) pressure.

• $P_2$ is the final pressure.

• $V_1$ is the original (initial) volume.

• $V_2$ is the final volume.

Substituting the given parameters into the formula, we have;

$788\times 0.235 = P_2 \times 0.115\\\\185.18 = 0.115P_2\\\\P_2 = \frac{185.18}{0.115} \\\\P_2 =1610.26\; Torr$

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