A gas initially at 4.0 L, 1.2 atm, and 66°C undergoes a change so that its final volume and temperature are 1.7 L and 42°C. What is its final pressure? Assume the number of moles remains unchanged.
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SOLUTION:
Step 1: List the given values.
To convert the temperature from degree Celsius to kelvin, add 273 to the temperature expressed in degree Celsius.
[tex]\begin{aligned} P_1 & = \text{1.2 atm} \\ V_1 & = \text{4.0 L} \\ T_1 & = 66^{\circ}\text{C} = \text{339 K} \\ V_2 & = \text{1.7 L} \\ T_2 & = 42^{\circ}\text{C} = \text{315 K} \end{aligned}[/tex]
Step 2: Calculate the final pressure using combined gas law.
[tex]\begin{aligned} P_2 & = \frac{P_1V_1T_2}{V_2T_1} \\ & = \frac{(\text{1.2 atm})(\text{4.0 L})(\text{315 K})}{(\text{1.7 L})(\text{339 K})} \\ & = \boxed{\text{2.6 atm}} \end{aligned}[/tex]
Hence, the final pressure is 2.6 atm.
[tex]\\[/tex]
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