Answer: 59.24 atm
Step-by-step explanation:
Given that:
Original Volume of gas V1 = 2.7L
Temperature T1 = 42.7°C
Convert Celsius to Kelvin
(42.7°C + 273 = 315.7K)
Pressure P1 = 684.9 torr
Final Volume V2 = 0.14 L
Final temperature T2 = 803.1°C
Convert Celsius to Kelvin
(803.1°C + 273 = 1076.1K)
Final pressure = ?
Then, apply the combined gas equation
(P1V1)/T1 = (P2V2)/T2
(684.9 torr x 2.7L)/315.7K = (P2 x 0.14L)/1076.1K
1849.23/315.7 = 0.14P2/1076.1
Then, cross multiply
1849.23 x 1076.1 = 315.7 x 0.14P2
1989956.403 = 44.198P2
Divide both sides by 44.198
1989956.403/44.198 = 44.198P2/44.198
45023.67 torr = P2
Now, convert the pressure in torr to atmosphere
If 760 torr = 1 atm
45023.67 torr = Z atm
Then, cross multiply
760 torr x Z = 45023.67 torr x 1 atm
Z = 45023.67 torr / 760 torr
Z = 59.24 atm
Thus, the new pressure of the gas will be 59.24 atm