A 5.00 L container contains #CH_4# at 35°C with a total pressure of 1.81 atm. What is the pressure of the gas when it expands to 25.0 L at 25°C?

Answer 1

Avery Adams

#(P_1V_1)/T_1=(P_2V_2)/T_2# #~=# #0.4*atm#

#(P_1V_1)/T_1=(P_2V_2)/T_2#

#P_2=(P_1V_1)/T_1xxT_2/V_2#

#=(1.81*atmxx5.00*Lxx298*K)/(308*Kxx25.0*L)# #=# #??atm#

It should be noted that I used absolute temperature because these issues always call for such measurements:

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Answer 2

Serenity Allen

Use the combined gas law to find the final pressure (P2). The formula is P1 * V1 / T1 = P2 * V2 / T2. Plug in the given values: P2 = (1.81 * 5.00 * (25 + 273)) / (35 + 273 * 25.0). Calculate to find the pressure of the gas when it expands.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.