A syringe filled with gas holds a volume of 35mL The pressure of the gas in the syringe is
105kPa and it is being held at a temperature of 22°C

If the syringe were warmed to 45°C but the volume were not changed what would be the new
pressure of the gas in the syringe?

if, instead the syringe were warmed to 45°C but the volume was allowed to increase while the
pressure remained constant predict the new volume of the syringe.

When we have a relation between the volume of a gas, the pressure, and the temperature participating together we can use the Combined Gas Law to solve the new pressure or volume.

What is Combined Gas Law?

The combined gas law shows the relation between Boyle's Law, Charles Law, and Gay-Lussac's Law and can be expressed by using the formula:

[tex]\mathbf{\dfrac{P_1V_1}{T_1}= \dfrac{P_2V_2}{T_2}}[/tex]

From the parameters given:

Initial volume = 35 mL
Initial Pressure = 105 kPa
Initial Temperature = 22°C = (273 + 22) K = 295 K

Final temperature = 45 °C = 318 K
Final volume = 35 mL
Final Pressure = unknown??

[tex]\mathbf{\dfrac{105 \times 35 }{295 }= \dfrac{P_2 \times 35}{318}}[/tex]

[tex]\mathbf{P_2= \dfrac{12.458 \times 318}{35}}[/tex]

[tex]\mathbf{P_2= 113 \ kPa}[/tex]

However, if the initial volume is increased let say to 50 mL and pressure is constant:

[tex]\mathbf{\dfrac{V_1}{T_1}= \dfrac{V_2}{T_2}}[/tex]

[tex]\mathbf{\dfrac{ 50 }{295 }= \dfrac{ x}{318}}[/tex]

[tex]\mathbf{x = \dfrac{ 318 \times 50 }{295 }}[/tex]

x = 54 mL

Therefore, the new volume of the syringe will also increase if the syringe were warmed to 45°C and the pressure remains constant.

Learn more about the combined gas Law here:

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