Answer:
786.88 mmHg
Step-by-step explanation:
From the question given above, the following data were obtained:
Initial temperature (T1) = 235 °C
Initial pressure (P1) = 743 mmHg
Volume = constant
Final temperature (T2) = 265 °C
Final pressure (P2) =..?
Next, we shall convert Celsius temperature to Kelvin temperature. This can be obtained as follow:
T(K) = T(°C) + 273
Initial temperature (T1) = 235 °C
Initial temperature (T1) = 235 °C + 273 = 508 K
Final temperature (T2) = 265 °C
Final temperature (T2) = 265 °C + 273 = 538 K
Finally, we shall determine the new pressure as illustrated below:
Initial temperature (T1) = 508 K
Initial pressure (P1) = 743 mmHg
Final temperature (T2) = 538 K
Final pressure (P2) =..?
P1/T1 = P2/T2
743/508 = P2/538
Cross multiply
508 × P2 = 743 × 538
508 × P2 = 399734
Divide both side by 508
P2 = 399734 / 508
P2 = 786.88 mmHg
Therefore, the new pressure of the gas is 786.88 mmHg