Answer:
[tex]\small \boxed{\sf \: Raised \: Pressure (P_2 )= 101.5649 \: ATM}[/tex]
Explanation:
Given:
P1 = 78.89 ATM
V1 = 12 litres
T1 = 70° C= 343.15 K
V2 = 10 litres
T2 = 95°C= 368.15 K
To find:
P2 = ?
Solution:
Using ideal gas equation,
[tex]PV = nRT[/tex]
Since the number of moles & Universal gas constant (R) is constant, the final relation that would be derived between initial & final variables.
(The only unit conversion needed is temperature because it was an addition factor, for other variables it will be cancelled out)
[tex] \frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2} \\ \\ \frac{78.89 \times 12}{343.15} = \frac{P_2 \times 10}{368.15} \\ \\ P_2 = \frac{78.89 \times 12 \times 368.15}{343.15 \times 10} \\ \\ \boxed{\sf \: P_2 = 101.5649 \: \: ATM}[/tex]
[tex] \small \sf \: Answer \rightarrow \: The \: pressure \: will \: raise \: to \: 101.5649 \: ATM[/tex]
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