Temperature

Volume

Top Answer

12.90

(Explanation): use charle's law for this one. V/T=V/T. we know the temperatures in both scenarios, and we're trying to solve for the volume in the beginning. Remember temperature in Kelvin! So, plug in what we know to get V/224.97K =29.164/508.59K. Now, cross-mulitply to solve for V. Equation now looks like this 508.59V=6561.02508. Now, divide by 508.59 on both sides to get 12.90042093. Round to 4 sig figs, 12.90 DONE!

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0(323 times 2)/3 = 273x/1 where x = v2646/3=273xx= (215 + 1/3)/273 = 8x10(-1) liters, or 0.8 liters.

- by the variation of the temperature- by the variation of the pressure

The volume of one mole of gas at a standard temperature and pressure is 22.4 liters. Multiply 22.4 liters by 0.25 moles to get a volume of 5.6 liters.

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

If temperature increases at a constant pressure the volume will increase. Temperature and volume both stick together T-V --->(DOWN)

3.5 litre if pressure is kept constant.

Then the volume will increase by a factor proportional to the absolute temperature. In other words, multiply the previous volume by (350/300).

Liters is a measurement of volume. 160 Liters is the volume.

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.

16.0 grams of O2 is equal to 0.5 moles, which has a volume of 11.2 liters at STP. 16.0 moles of O2 has a volume of ?æ358 liters.

Of course. But at STP, any gas has a standard volume of 22.4 Liters.

length = centimeters, or meters. volume = liters. temperature = Celsius, or Kelvin. mass = grams, or kilograms.

It depends upon the substance and the temperature. For water at room temperature the volume would be 0.0125L

Under constant pressure the new volume is (new temp/original temp) x original volume. You first need to convert temp to Kelvin by adding 273 degrees new volume = (771.3) x 297/352 = 650.8 ml

Pressure and temperature. As pressure increases, volume decreases; as temperature increases, volume increases with it. At standard temperature and pressure (1 atm, 273 degrees Kelvin), one mole of a gas (6.022 x 1023 particles) has the volume of 22.4 liters.

An experimental gas law is the Charles Law. The formula used is original volume/original temperature= new volume/new temperature. The law describes expansion of gases with heat.

4.5 liters at STP (standard temperature and pressure)

54 liters at STP (standard temperature and pressure)

0.48 liters at STP (standard temperature and pressure)

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