A sample of argon gas at a pressure of and a temperature of, occupies a volume of. If the gas is heated at constant pressure until its volume is, the temperature of the gas sample will be °C.
Answer:
Step 1: Explanation:
We know the ideal gas equation, PV = nRT
where,
R=universal gas constant,T=temperature ,P=pressure,V=volume,n=moles.
=> PV = nRT
=> V/T=K where, K = constant [since nR and Pressure all are assume constant]
=> So, we have V1/T1 = V2/T2.
Step 2: Extract the data from the question
Given,
V1 = 805 mL
T1= 137 °C = ( 137 +273.15) K = 410.15 K
V2= 1000 mL
T2 = we need to find and
Step 3: Calculation
By using above equation
V1/T1 = V2/T2.
=> T2 = V2T1 / V1
=> T2 = ( 1000 mL × 410.15 K) / 805 mL= 509.5 K = 236.35 °C
[ we got 509.5 K => 509.5 K = ( 509.5 K -273.15) °C = 236.35 °C ]
Hence, the new temperature is 236.35 °C
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