2.00 liters of hydrogen, originally at 25.0 °C and 750.0 mm of mercury, are heated until a volume of 20.0 liters and a pressure

Question

22 days ago

8

of 3.50 atmospheres is reached. What is the new temperature?

1 answer:

eduard [2.5K] · Answer 1 · 2026-03-14T15:04:01+03:00

Response: The updated temperature stands at 10643 K

Clarification:

The combined gas law integrates Boyle's law, Charles's law, and Gay-Lussac's law.

The equation for this law is given by:

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

where,

$P_1$ = initial gas pressure = 750.0 mm Hg = 0.98 atm (760mmHg=1atm)

$P_2$ = final gas pressure = 3.50 atm

$V_1$ = initial gas volume = 2.00 L

$V_2$ = final gas volume = 20.0 L

$T_1$ = initial gas temperature = $25.0^oC=273+25.0=298.0K$

$T_2$ = final gas temperature =?

Now substituting all the stated values into the equation, we obtain:

$\frac{0.98\times 2.00}{298.0K}=\frac{3.50\times 20.0}{T_2}$

$T_2=10643K$

Thus, the new temperature results in 10643 K