Answer:
The temperature of the gas contained in the container is -259.35° C
Explanation:
To find the unit of degrees in Celsius (° C) in this case, the ideal gas law equation is used.
PV = nRT
Where P is the pressure, V is the volume, T is the temperature, n is the number of moles, and R is the universal gas constant.
Solving for T would be: PV / nR
T = ( 1.4113 atm * 2.00 L ) / ( 2.49 mol * 0.08205746 atm * L / mol * K )
T = 2.8226 / 0.2043
T = 13.8K = -259.35 ° C
Answer:
The Celsius temperature of the gas is -259.34 ° C
Explanation:
To answer the question, we note that the universal gas equation can be expressed as follows;
P·V = n·R·T
Therefore;
[tex]T = \frac{P \cdot V}{R \cdot n}[/tex]
Where:
n = Number of moles = 2.49 mol
P = Pressure = 143 kPa = 143000 Pa
V = Volume = 2.00 L = 0.002 m³
T = Temperature in Kelvin, K = Required
R = Universal Gas Constant = 8.3145 J/(mol·K)
Plugging in the values, we have;
[tex]T = \frac{143000 \times 0.002 }{8.3145 \times 2.49 } = 13.81 \, K[/tex]
Hence the temperature of the gas = 13.81 K
Converting the Kelvin temperature to Celsius temperature, we have
Celsius temperature = Kelvin temperature - 273.15
Therefore, 13.81 K to Celsius temperature gives;
13.81 - 273.15 = -259.34 ° C.
