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Q: What is the final volume, in liters, of the gas when measured at 24 ∘C and 635 mmHg, when n is constant?

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This problem can be solved with the ideal gas law. The original pressure and volume of the container are proportional the final pressure and volume of the container. The original pressure was 1 atmosphere and the original volume was 1 liter. If the final volume is 1.8 liters, then the final pressure is 0.55 atmospheres.

This question makes no sense because pressure is not measured in mL.

You can calculate pressure and temperature for a constant volume process using the combined gas law.

BOYLES LAW The relationship between volume and pressure. Remember that the law assumes the temperature to be constant. or V1 = original volume V2 = new volume P1 = original pressure P2 = new pressure CHARLES LAW The relationship between temperature and volume. Remember that the law assumes that the pressure remains constant. V1 = original volume T1 = original absolute temperature V2 = new volume T2 = new absolute temperature P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature IDEAL GAS LAW P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature Answer BOYLES LAW The relationship between volume and pressure. Remember that the law assumes the temperature to be constant. or V1 = original volume V2 = new volume P1 = original pressure P2 = new pressure CHARLES LAW The relationship between temperature and volume. Remember that the law assumes that the pressure remains constant. V1 = original volume T1 = original absolute temperature V2 = new volume T2 = new absolute temperature P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature IDEAL GAS LAW P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature

Pressure is halved when ONLY volume is doubled (n and T are constant).Remember the General Gas Law:p.V = n.R.T(in which R=general gas constant)

If pressure is held constant, volume and temperature are directly proportional. That is, as long as pressure is constant, if volume goes up so does temperature, if temperature goes down so does volume. This follows the model V1/T1=V2/T2, with V1 as initial volume, T1 as initial temperature, V2 as final volume, and T2 as final temperature.

1.83

P V = k T, so at constant temperature, PV is constant Initial PV = (102.5 x 3.67) = 376.175 ====> At constant temp, V = (376.175 / P) Final P = 100.9. Final V = (376.175 / 100.9) = 3.7282 L (rounded)

60

Molarity (M) is defined as moles of solute/liters of solution. Assuming the final volume is 500 ml (0.5 liters), then M = 1.2 moles/0.5 liters = 2.4 M

What? Pressure cannot be measured in m or in mL. Please check you homework and resubmit the correct question.

42.8 grams of KIO3 and add H2O until the final homogeneous solution has a volume of 2.00 liters