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NISA [10]
3 years ago
14

A container holds 500. mL of CO2 at 20.° C and 735 torr. What will be the volume of the CO2 if the pressure is increased to 807

torr? (0.456 L)
Chemistry
1 answer:
Alinara [238K]3 years ago
5 0

Answer:- 0.456 L

Solution:- Looking at the given information, only volume and pressure are changing and the temperature is constant. We know that, at constant temperature, the volume of the gas is inversely proportional to the pressure.

P_1V_1=P_2V_2

P_1 = 735 torr

P_2 = 807 torr

V_1 = 500. mL

V_2 = ?

Let's plug in the values in the equation and solve it for final volume.

735torr(500.mL)=807torr(V_2)

V_2=\frac{735torr(500.mL)}{807torr}

V_2=456mL

since, 1 L = 1000 mL

456mL(\frac{1L}{1000mL})

= 0.456 L

So, the volume of carbon dioxide at the new pressure will be 456 mL or 0.456 L.

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