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A gas is initially confined to a 1.00 L vessel at 3.00 atm of pressure. A valve connecting the 1.00 L vessel to a 3.00 L vessel is opened and the gas expands. What is the final pressure in atm of the gas after the valve is opened, assuming that the volume of the connecting tube is negligible and there is no temperature change?

a. 0.250 atm
b. 0.500 atm
c. 0.750 atm
d. 1.00 atm
e. None of these choices

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Answer:

c. 0.750 atm .

Explanation:

Hello!

In this case, since the two vessels have different volume, we can see that the gas is initially at 3.00 atm into the 1.00-L vessel, but next, it is allowed to move towards the 3.00-L vessel, meaning that the final volume wherein the gas is located, is 4.00 L; therefore, we use the Boyle's law to compute the final pressure:

[tex]P_2V_2=P_1V_1\\\\P_2=\frac{P_1V_1}{V_2} \\\\P_2=\frac{3.00atm*1.00L}{4.00L}\\\\P_2=0.750atm[/tex]

Therefore the answer is c. 0.750 atm .

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