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A piston with a volume of 847.1 mL is filled with 0.187 moles of a gas at 357.8 K and 305.7 mm Hg. The piston is then compressed by 228.1 mL and cooled to 205.2 K. What is the pressure (in atm) of the piston under these final conditions?

2 Answers

1 vote

Answer:

Step-by-step explanation:

p(i)*v(i)/t(i)=p(f)*v(f)/t(f)

plug and chug

User MyNameIsKhan
by
7.8k points
3 votes

Answer : The pressure (in atm) of the piston under these final conditions is, 0.857 atm

Explanation :

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,


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

where,


P_1 = initial pressure of gas = 305.7 mmHg


P_2 = final pressure of gas = ?


V_1 = initial volume of gas = 847.1 mL


V_2 = final volume of gas = 228.1 mL


T_1 = initial temperature of gas = 357.8 K


T_2 = final temperature of gas = 205.2 K

Now put all the given values in the above equation, we get:


(305.7mmHg* 847.1mL)/(357.8K)=(P_2* 228.1mL)/(205.2K)


P_2=651.1mmHg=0.857atm

conversion used : (1 atm = 760 mmHg)

Thus, the pressure (in atm) of the piston under these final conditions is, 0.857 atm

User Mahendra Rathod
by
7.6k points
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