A 0.286 g sample of carbon dioxide, CO 2 , has a volume of 565 mL and a pressure of 455 mmHg . What is the temperature, in kelvins and degrees Celsius, of the gas? Part A What is the temperature, in degrees Celsius, of the gas? Part B What is the temperature, in kelvins, of the gas?
Following is the - complete Answer -&- Explanation: for the given: Question: in....typed format...
Answer(s):
Explanation:
Following is the complete Explanation: for the above: Answer(s).
Using the above stated: molar mass: of carbon di-oxide ; CO2, and the above stated mass of CO2, we will get the following :
Moles of CO2 : nco2 = ( mass of CO2 ) / ( molar mass of CO2 ) = ( 0.286 g ) / ( 44.01 g/mol )
= 0.0065 mol ( moles, approx. )
We can use the Ideal Gas Law: to determine the value of temperature : of the gas: i.e. CO2 ....
Ideal Gas Law: P x V = n x R x T -----------------------------Equation - 1
Where:
We know:
Ideal Gas Law: P x V = n x R x T -----------------------------Equation - 1
Plugging in values, in Equation - 1: we will get the following:
T = P x V / ( n x R )
T = [( 455.0 Torr ) x ( 0.565 L ) ] / [ ( 0.0065 mol ) x ( 62.364 L. Torr / ( mol. K ) ) ] = 634.18 K ( Kelvin )
Therefore: T = 634.18 K = ( 634.18 - 273.15 ) = 361.03 oC
Therefore: we will get the following: answer(s):
Part - (B): Temperature of the gas ( CO2 ) in Kelvin : T = 634.18 K ( Kelvin )
AND:
Part - ( A ): Temperature of the gas ( CO2 ) in oC : T = 361.03 oC ( deg. C )
A 0.286 g sample of carbon dioxide, CO 2 , has a volume of 565 mL...
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