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The pressure is changed from 500 kPa to 250 kPa. What would you expect the new volume to be if the initial volume is 200 mL?
Zachary Kronlage
400 mL
(Explanation): again boyle's law PV=PV. Since the pressure is halved (500 to 250), then the volume must be doubled in order to maintain this equation. 200 x2=400 so that's the answer
Zachary Kronlage
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How does the pressure of a container change as the volume is changed?
In a small volume container the pressure is higher.
What volume would you expect the gas to occupy if the pressure is increased to 40 kPa?
The volume you would expect the gas to occupy if the pressure is increased to 40 kPa would be 50 liters.
Is it possible for a balloon with an initial pressure of 200.0kPa to naturally expand four times its initial volume when the temperature remains constant and atmospheric pressure is 101.3kPa?
svfdvf
As the pressure of a gas at 760 torr is changed to 380 torr at a constant temperature the volum of the gas will?
Boyle's law states that pressure is indirectly proportional to the volume. There fore as the pressure of a gas at 760 torr is changed to 380 torr, the volume will increase. Boyle's Law: P1 x V1 = P2 x V2 Rearranging leads to: P1 / P2 = V2 / V1 Substituting our values: 760 / 380 = V2 / V1 Thus the final volume will be twice the initial volume.
The gas with an initial volume of 24.0 L at a pressure of 565 mmHg is compressed until the volume is 16.0 L What is the final pressure of the gas?
500. mmHg
What is Charles law and boyles 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
How to calculate final pressure when given initial pressure and initial temp and also final temp and know that it's a constant volume process from initial state?
You can calculate pressure and temperature for a constant volume process using the combined gas law.
How does the pressure of a container change as the volume is changed?
In a small volume container the pressure is higher.
What is its volume when the pressure is tripled?
1/3 of the initial volume (Boyle-Mariotte law).
According to ideal gas eqation if pressure is double to initial pressure then what happens to the volume?
It would be half of the original volume. As you reduce the volume the pressure would increase and at half the original volume the pressure would be doubled.
What volume would you expect the gas to occupy if the pressure is increased to 40 kPa?
The volume you would expect the gas to occupy if the pressure is increased to 40 kPa would be 50 liters.
Is it possible for a balloon with an initial pressure of 200.0kPa to naturally expand four times its initial volume when the temperature remains constant and atmospheric pressure is 101.3kPa?
svfdvf
As the pressure of a gas at 760 torr is changed to 380 torr at a constant temperature the volum of the gas will?
Boyle's law states that pressure is indirectly proportional to the volume. There fore as the pressure of a gas at 760 torr is changed to 380 torr, the volume will increase. Boyle's Law: P1 x V1 = P2 x V2 Rearranging leads to: P1 / P2 = V2 / V1 Substituting our values: 760 / 380 = V2 / V1 Thus the final volume will be twice the initial volume.
What must the pressure and volume be if the pressure of its container is reduced to half its original size?
initial volume = V1 final volume = V2 initial pressure = P1 final pressure = P2 = (1/2)P1 P1V1 = P2V2 P1V1 = (1/2)P1V2 P1 cancels; V1 = (1/2)V2 V2 = 2V2.
The gas with an initial volume of 24.0 L at a pressure of 565 mmHg is compressed until the volume is 16.0 L What is the final pressure of the gas?
500. mmHg
What happens to the volume of solids liquids and gases when they cool?
Solids- stays the same Liquids- stays the same Gases- decreases You can use the formula PV/T=P2V2/T2 P=initial pressure V=initial volume T=initial temp P2=final pressure V2=final volume T2=final temp
What is the final pressure of a system (ATM) that has the volume increased from 0.75 L to 3.1L with an initial pressure of 1.25 ATM?
1.1
