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A gas balloon has a volume of 99.71 liters when the temperature is 44.7 °C and the pressure is 707.2 mmHg. What would its volume be at 10.4 °C and 602.6 mmHg?

Give your answer in L to the tenths place. Do not put units in the answer space.

Sagot :

julianandres98moncay

Applying Charles's law and Boyle's law together, we can combine them into the ideal gas law:

PV = nRT

where:

* P = Pressure (mmHg)

* V = Volume (L)

* n = Number of moles (assumed constant)

* R = Gas constant (0.08206 L atm / K mol)

* T = Temperature (K)

We can rearrange the equation to find the final volume (V₂) at the new temperature (T₂) and pressure (P₂):

V₂ = V₁ * (T₂ / T₁) * (P₁ / P₂)

Plugging in the known values:

V₂ = 99.71 L * ((10.4 + 273.15) K / (44.7 + 273.15) K) * (707.2 mmHg / 602.6 mmHg)

V₂ ≈ 107.7 L

Therefore, the volume of the gas balloon at 10.4 °C and 602.6 mmHg would be approximately 107.7 liters.

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