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I have a balloon that can hold 100. liters
of air. If I blow up this balloon with 3.0
moles of oxygen gas at a pressure of 1.0
atmosphere, what is the temperature of
the balloon?

Sagot :

Drpelezoidn

Answer:

T = 4.062V

Explanation:

from PV = nRT => T = PV/RT

P = 1 atm

V = Final Volume

n = 3 moles

R = 0.08206 L·atm/mol·K

T = ?

T = 1 atm · V(Liters)/(3 moles)(0.08206L·atm/mol·K) = 4.062·V(final) Kelvin

Eduard22slyidn

The temperature of the balloon is 406 K

We'll begin by listing out what was given from the question. This is shown below:

Volume (V) = 100 L

Mole of oxygen (n) = 3 moles

Pressure (P) = 1 atm

Temperature (T) =?

We can obtain the temperature of the balloon by using the ideal gas equation as shown below:

PV = nRT

NOTE:

P is the pressure.

V is the volume.

n is the number of mole

R is the gas constant (0.0821 atm.L/Kmol)

T is the temperature.

Applying the ideal gas equation, we have:

PV = nRT

1 × 100 = 3 × 0.0821 × T

100 = 0.2463 × T

Divide both side by 0.2463

T = 100 / 0.2463

T = 406 K

Therefore, the temperature of the balloon is 406 K

Learn more: https://brainly.com/question/17046345

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