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what’s the temperature in Celsius of an unknown gas if 0.944 moles is contained in a 3.75 liter container with a pressure of 247.4 ka?

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To calculate the temperature of the gas, we can use the Ideal Gas Law equation:

PV = nRT

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

We can rearrange this equation to solve for T:

T = PV/nR

where:

P = 247.4 kPa (we convert from ka to kPa)

V = 3.75 L

n = 0.944 mol

R = 8.31 J/(mol*K) (the ideal gas constant)

Substituting these values into the equation, we get:

T = (247.4 kPa * 3.75 L) / (0.944 mol * 8.31 J/(mol*K))

Simplifying this expression, we get:

T = 93.6 K

Therefore, the temperature of the gas is 93.6 Kelvin. To convert this to Celsius, we can subtract 273.15 from the Kelvin temperature:

T (Celsius) = 93.6 K - 273.15 = -179.55 °C (rounded to two decimal places)

Therefore, the temperature of the gas is approximately -179.55 degrees Celsius.

User Arcayne
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