Answer: 41 atm
Explanation:
Given that:
Original Volume of gas V1 = 2.9L
Temperature T1 = 32.7°C
Convert Celsius to Kelvin
(32.7°C + 273 = 305.7K)
Pressure P1 = 645.3 torr
New Volume V2 = 0.23 L
New temperature T2 = 894.7°C
Convert Celsius to Kelvin
(894.7°C + 273 = 1167.7K)
New pressure = ?
Then, apply the combined gas equation
(P1V1)/T1 = (P2V2)/T2
(645.3 torr x 2.9L)/305.7K = (P2 x 0.23L)/1167.7K
1871.37 / 305.7 = 0.23P2 / 1167.7
To get P2, Cross multiply
1871.37 x 1167.7 = 305.7 x 0.23P2
2185198.749 = 70.311P2
Divide both sides by 70.311
2185198.749/70.311 = 70.311P2/70.311
31079.045 torr = P2
Now, convert pressure in torr to atmosphere
Since 760 torr = 1 atm
31079.045 torr = Z
cross multiply
760 torr x Z = 31079.045 torr x 1 atm
Z = 31079.045 torr / 760 torr
Z = 40.89 atm (Round to the nearest whole number as 41 atm)
Thus, new pressure of gas is 41 atm
