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ValentinkaMS [17]
2 years ago
10

A sample of a gas in a 4 L container at 300 K has a pressure of 1 atm. If the temperature is increased to 600 K and the volume i

s decreased to 2 L, the pressure is likely to be closest to which of the following?
0.5 atm
в
1 atm
с
2 atm
D
4 atm
Chemistry
1 answer:
icang [17]2 years ago
6 0

Answer:

Explanation:

Did u ever get the answer?

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What we're looking for here is the gas sample's molar mass given its mass, pressure, volume, and temperature. Recalling the gas law, we have

PV = nRT or
n = \frac{PV}{RT}

where R is <span>0.08206 L atm / mol K, P is the given pressure, T is the temperature, and V is the volume.

Before applying the values given, it is important to make sure that they are to be converted to have consistent units with that of R. 
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Thus, we have

P = 736/ 729 = 0.968 atm
T = 28 + 273.15 = 301.15 K
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Now, applying these converted values into the gas law, we have

n = \frac{(0.968 atm)(0.250 L)}{(0.08206 L.atm/mol.K)(301.15 K)}
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Given that the mass of the sample is 0.430 g, we have

molar mass = \frac{mass}{number of moles} 
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Thus, the gas sample has a molar mass of 43.9 g/mol.
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