Activity:
0.01 kg of a certain perfect gas occupies a volume of 0.003m3 at a pressure of 7 bar and a temperature of 131°C. Calculate the molar mass of the gas. When the gas is allowed to expand until the pressure is 1 bar the final volume is 0.02m3. Calculate the final temperature.
p1V1=mRT1R=p1V1mT1T1=131+273=404 KR=7×105×0.0030.01×404=520 N⋅m/kgR=R0MM=R0RM=8314520=16p_1V_1=mRT_1 \\ R=\frac{p_1V_1}{mT_1} \\ T_1=131+273=404 \;K \\ R= \frac{7 \times 10^5 \times 0.003}{0.01 \times 404} = 520 \; N \cdot m/kg \\ R=\frac{R_0}{M} \\ M = \frac{R_0}{R} \\ M=\frac{8314}{520}=16p1V1=mRT1R=mT1p1V1T1=131+273=404KR=0.01×4047×105×0.003=520N⋅m/kgR=MR0M=RR0M=5208314=16
Molecular weight = 16
p2V2=mRT2T2=p2V2mRT2=1×105×0.020.01×520=384.5 Kp_2V_2=mRT_2 \\ T_2 = \frac{p_2V_2}{mR} \\ T_2= \frac{1 \times 10^5 \times 0.02}{0.01 \times 520} = 384.5 \;Kp2V2=mRT2T2=mRp2V2T2=0.01×5201×105×0.02=384.5K
Final temperature =384.5−273=111.5 °C= 384.5-273=111.5 \;°C=384.5−273=111.5°C
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