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alisha [4.7K]
3 years ago
13

5.00 L of a gas is collected at 22.0 'C and 745.0 mmHg . When the temperature increases to 35'C what is the new pressure

Physics
1 answer:
Inessa [10]3 years ago
3 0

Answer:

The new pressure is 777.926 mmHg.

Explanation:

We use the ideal gas equation

PV = nrT.

where P, V , n, and T are the pressure, volumes, moles, and temperature of the gas respectively. r is the gas constant r = 8.3145\: j*mol^{-1}*K^{-1}.

Initially, for the gas

V = 5L = 0.005m^3

P = 745.0 \:mmHg  = 99325.2\: Pa

T = 22^oC = 295\:K.

therefore, the number of moles n is

(99325.2\:Pa)(0.005m^3) = n( 8.3145\: j*mol^{-1}*K^{-1})(295K)

n = \dfrac{(99325.2\:Pa)(0.005m^3)}{( 8.3145\: j*mol^{-1}*K^{-1})(295K)}

n= 0.2025

Now, when the temperature rises to 35°C, (assuming constant volume) we have

P = \dfrac{0.2025mol*8.3145\: j*mol^{-1}*K^{-1}308K }{0.005m^3}

P = 103715.1 \: Pa

or in mmHg this is

\boxed{P = 777.926\:mmHg}

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