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2 years ago

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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?

1 answer:

dedylja [7]2 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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<u>Answer:</u> The pH of the solution after addition of KOH is 3.84

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To calculate the pH of acidic buffer, we use the equation given by Henderson Hasselbalch:

$pH=pK_a+\log(\frac{[salt]}{[acid]})$

$pH=pK_a+\log(\frac{[HCOO^-]}{[HCOOH]})$

We are given:

$pK_a$ = negative logarithm of acid dissociation constant of formic acid = 3.75

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Hence, the pH of the solution after addition of KOH is 3.84

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