I don’t understand the question
Using the ideal gas law (PV = nRT), you can calculate the initial and final number of moles of CO2. Given that the temperature remains constant, the ratio of the initial volume to final volume is equal to the ratio of the initial pressure to the final pressure. Applying this ratio to the initial volume of 1.25 liters will give you the final volume.
To calculate the new volume of the hydrogen gas, you can use Charles's Law, which states that the volume of a gas is directly proportional to its temperature (at constant pressure). You would first convert the temperatures to Kelvin (373 K and 473 K), then use the ratio of the initial and final temperatures to find the new volume. The new volume of the gas would be 35 liters.
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.
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)
Molarity = moles of solute / liters of solution. First, calculate the moles of NaOH using its molar mass. Then, divide the moles by the final volume in liters (3.00 L) to find the molarity.
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
1.83
Assuming pressure is constant, like you said, volume and temperature have a direct relationship. As temperature increases, volume increases; as temperature decreases, volume decreases. Setting up a algebraic direct proportion, you get approximately 3.84 liters for the balloon at 285 degrees K.
PV = constant
In Boyle's Law, p2 represents the final pressure when a gas undergoes a change in volume at constant temperature. The law states that the initial pressure (p1) times the initial volume (V1) is equal to the final pressure (p2) times the final volume (V2), where p1V1 = p2V2.