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PilotLPTM [1.2K]
3 years ago
6

Calculate the volume the gas will occupy if the pressure is increased to 1.89 atmatm while the temperature is held constant. Exp

ress the answer in liters to three significant figures.
Chemistry
1 answer:
Y_Kistochka [10]3 years ago
6 0

Question is incomplete, complete question is :

A fixed quantity of gas at 21°C exhibits a pressure of 758 torr and occupies a volume of 5.42 L . Calculate the volume the gas will occupy if the pressure is increased to 1.89 atm while the temperature is held constant.

Answer:

The final volume of the gas will be 2.86 L.

Explanation:

initial pressure of the gas = P_1=758 Torr=\frac{758}{760} atm=0.997 atm

initial volume of the gas = V_1=5.42 L

Final pressure of the gas = P_2=1.89 atm

Final volume of the gas = V_1=?

Applying Boyle's law;

P_1V_1=P_2V_2 ( at constant temperature)

V_2=\frac{P_1V_1}{P_2}=\frac{0.997 atm\times 5.42 L}{1.89 atm}

V_2=2.86 L

The final volume of the gas will be 2.86 L.

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A solution has a pOH of 7. 1 at 10∘c. Then the pH of the solution given that kw=2. 93×10−15 at this temperature is 7.4 .

It is given that,

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learn more about pH value:

brainly.com/question/12942138

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