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Len [333]
3 years ago
8

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

of 3.50 atmospheres is reached. What is the new temperature?
Chemistry
1 answer:
dedylja [7]3 years ago
6 0

Answer:  The new temperature is 10643 K

Explanation:

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

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

where,

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

P_2 = final pressure of gas = 3.50 atm

V_1 = initial volume of gas = 2.00 L

V_2 = final volume of gas = 20.0 L

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

T_2 = final temperature of gas = ?

Now put all the given values in the above equation, we get:

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

T_2=10643K

Thus the new temperature is 10643 K

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