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What is the pressure, in bar, when 1.90moles of an ideal gas occupy 76.2L at 571.7K?

User Loki L
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1 Answer

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We can use the ideal gas law to solve for the pressure:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

First, we need to convert the temperature from Celsius to Kelvin:

571.7 K = 298.55°C + 273.15 = 871.7 K

Now we can plug in the values and solve for P:

P = nRT/V

P = (1.90 mol)(0.08206 L·atm/mol·K)(871.7 K)/(76.2 L)

P = 37.9 atm

Finally, we convert the pressure from atm to bar by dividing by 1.01325:

P = 37.9 atm / 1.01325 = 37.4 bar

Therefore, the pressure is 37.4 bar when 1.90 moles of an ideal gas occupy 76.2 L at 571.7K.

User Eric Su
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