Question

If 9.76 moles of an ideal gas has a pressure of 1.84 atm, and a volume...

If 9.76 moles of an ideal gas has a pressure of 1.84 atm, and a volume of 70.61 L, what is the temperature of the sample in degrees Celsius?

We have to use ideal gas equation here

the equation is PV=nRT

Where

Here

• P is the pressure of the gas in atm
• V is the volume in lit
• n is the number of moles of gas present in the sample
• R is the universal gas constant, equal to 0.0821 atm L / mol K
• T is the absolute temperature of the gas in K

now rearrange the equation for T

PV=nRT

T = PV / nR

lets put the values in formula

T = (1.84 atm * 70.61 L) / 9.76 moles * 0.0821 atm L / mol K

T = 129.92 / 0.8013

T= 162.14 K

now we have to convert Kelvin to degrees Celsius

formula for this is

Kelvin = 273.15 + degrees Celsius

degrees Celsius= Kelvin - 273.15

degrees Celsius = 162.14 - 273.15

degrees Celsius =-111.01

So our final answer is -111.01 oC

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