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Arte-miy333 [17]
3 years ago
15

How many miles of a gas at 100 c does it take to fill a 1.00 l flask to a pressure of 152kPa

Chemistry
1 answer:
Hatshy [7]3 years ago
5 0

The complete question is as follows: How many moles of a gas at 100 c does it take to fill a 1.00 l flask to a pressure of 152kPa

Answer: There are 0.0489 moles of a gas at 100^{o}C is required to fill a 1.00 l flask to a pressure of 152kPa.

Explanation:

Given: Volume = 1.00 L,    

Pressure = 152 kPa (1 kPa = 1000 Pa) = 152000 Pa

Convert Pa into atm as follows.

1 Pa = 9.86 \times 10^{-6} atm\\152000 Pa = 152000 \times \frac{9.86 \times 10^{-6}atm}{1 Pa}\\= 1.5 atm

Temperature = 100^{o}C = (100 + 273) K = 373 K

Using the ideal gas formula as follows.

PV = nRT

where,

P = pressure

V = volume

n = no. of moles

R = gas constant = 0.0821 L atm/mol K

T = temperature

Substitute the values into above formula as follows.

PV = nRT\\1.5 atm \times 1.0 L = n \times 0.0821 L atm/mol K \times 373 K\\n = \frac{1.5 atm \times 1.0 L}{0.0821 L atm/mol K \times 373 K}\\n = 0.0489 mol

Thus, we can conclude that there are 0.0489 moles of a gas at 100^{o}C is required to fill a 1.00 l flask to a pressure of 152kPa.

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