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An oxygen tank contains oxygen at a pressure of 70 kPa When the pressure drops to 36 kPa the temperature increases from 300 K to 350 K If the initial volume is 9 L what is the final volume?
Vanessarojo
use the ideal gas last pv=nrt n= same for each one and R=8.314 j/mol*k
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∙ 15y ago
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What is p2 in boyles law?
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.
What is initial temperature?
This is the temperature at which an experiment begins.
A 2 liters tank contains air at 1atm and 20 degrees celsius.the tank is sealed and heated until the pressure is 3 atm.what is the temperature in degrees celsius?
Using the ideal gas law, (PV = nRT), we can solve for the final temperature using the initial conditions and new pressure. Rearranging the equation to solve for T, we get (T = (P2/P1) * T1), where T1 is the initial temperature. Substituting the values, we find the final temperature to be 80 degrees Celsius.
What is steam temperature after adiabatic expansion?
The steam temperature after adiabatic expansion depends on the specific conditions of the expansion process, such as initial temperature, pressure, and volume. During adiabatic expansion, the internal energy of the steam decreases, causing its temperature to drop. The final temperature can be determined using the appropriate thermodynamic equations.
What is the formula of Boyles law?
The mathematical equation for Boyle's law is PV = k or you could say P1V1=P2V2. P IS the pressure of the system. V is the volume of the gas. k is a constant value representative of the pressure and volume of the system. **It just states that pressure and volume are inversely proportional when temperature is held constant (does not change). In other words, as volume increases pressure decreases and vice-versa (when temperature is constant).** Also, an easy way to remember all of the laws (Boyle's, Charles', and Gay-Lussac's) is to remember one equation: The Ideal Gas Equation, which happens to be PV=nRT. P=pressure, V=volume, n=number of moles, R=constant (varies with certain units, for example, when using torrs or mm Hg it would equal 62.4), and T=temperature. You can make basic assumptions from this equation, for example, you know that when temperature is held constant that if pressure increases volume must decrease (which happens to be Boyle's Law).
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
Describe the relationship between temperature and pressure?
The relationship between temperature and pressure is not named after a specific person, like Boyle's or Charles' Laws, but states that the relationship between the temperature and pressure of a gas (usually as observed in a rigid container) is direct. Therefore, as temperature increases, pressure does too.This is Gay-Lussac's law.The temperature and pressure of gasses are related. As the pressure increases the temperature also increases, and vice verse. As the pressure decreases the temperature gets colder.The ideal-gas law may be expressed as PV=nRT.Absolute temperature TNumber of moles (a measure of the number of molecules) nVolume VPressure PRydberg's constant R (some value that makes the numbers and the units work)Obviously, from the equation, you could half the temperature and keep the pressure the same, if, for example, you cut the volume in half. Or you could half the temperature and double the number of moles, and the pressure wouldn't change.
What happens when a gas is compressed keeping the temperature 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.
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?
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Which container contains water with lower initial temperature?
You think probable to a Dewar container.
Why the temperature of the water increases from trial one to trial three?
During the time water absorb heat from the atmosphere if the initial temperature was lower.
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.
What effect does the initial temperature of the water have on change in temperature of the water after the hot metal is added?
When hot metal is added into the water then the metal looses its energy into the water and this heat is gained by the water, so the temperature gets increases when hot metal added into it i.e final temperature is greater than initial temperature of water.
If i have the initial and after temperature how would i be able to find the change in temperature?
You subtract the initial from the after, and the result is the change. If the initial temperature is 50º and the after is 70º, then the change is +20º.
What can you conclude about how the volume of given mass of gas changes as its pressure increases?
Pressure has no effect on the mass of a given sample of gas. Whatever the initial mass is, it won't change, regardless of the pressure, unless you let more gas in or let some escape.
What is meant by initial temperature rise of IC?
A: As power is turn on the temperature of the IC is at ambient temperature or the initial temperature then becomes the increase in temperature due to heating.
What would be the pressure in mm Hg if this gas was allowed to expand to 975 ml at a constant temperature?
This cannot be answered without an initial volume or pressure. But the final pressure of an expansion of a gas can be determined by the following formula. PV/T = P'V'/T' where P = pressure absolute V = volume T = temperature absolute ( ' ) indicates the new pressure, volume and temperature because the temperature is constant this can be reduced to PV = P'V' or P' = PV/V'
