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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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For the given equation :

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The molar mass of H2O is 18.01 g/mol. The molar mass of O2 is 32.00 g/mol. What mass of H2O, ins grams, must react to produce 50
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Answer:

56.28 g

Explanation:

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You have to use stoichiometry for the next part.  Looking at the equation, you can see that for every 2 moles of H₂O, 1 mole of O₂ is produced.  Convert from moles of O₂ to moles of H₂O using this relation.

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Convert to significant figures.

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