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a 150-g mass of krypton (molar mass 83.8 g/mol) occupies 15.0 l at a pressure of 210 kpa. what temperature is this sample of gas at in kelvin?

User Drdrej
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Final answer:

Using the ideal gas law and substituting the given values, the temperature of the 150-g mass of krypton at a pressure of 210 kPa and volume of 15.0 L is approximately 223.3 Kelvin.

Step-by-step explanation:

To find the temperature of a 150-g mass of krypton that occupies 15.0 L at a pressure of 210 kPa, we can use the ideal gas equation: PV = nRT, where P is pressure, V is volume, n is the number of moles of gas, R is the ideal gas constant, and T is temperature in Kelvin.

First, we calculate the number of moles (n) of krypton using its mass (m) and molar mass (M):

n = m / M = 150 g / 83.8 g/mol ≈ 1.789 moles

Next, we substitute the values into the ideal gas equation, solving for T:

PV = nRT ⇒ T = PV / (nR)

We use the value of R when the pressure is in kPa, which is 8.314 (L·kPa)/(K·mol).

T = (210 kPa) (15.0 L) / (1.789 moles) (8.314 L·kPa/K·mol)

T ≈ 223.3 K

Therefore, the temperature of the krypton gas under the given conditions is approximately 223.3 Kelvin.

User Haza
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