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What if gas is in a sealed container has a pressure of 50 k pa at 300 k what will the pressure be if the temperature rises 360 k?
60kpa
How valid is the assumption that the initial temperature of the steam is 100 degrees celsius?
The assumption that the initial temperature of steam is 100 degrees Celsius is generally valid when referring to saturated steam at atmospheric pressure. However, it's important to consider that the temperature of steam can vary depending on the pressure or if it is superheated. Additional information or measurements may be needed to confirm the exact initial temperature of the steam in a specific scenario.
What shows the relationship between the pressure and volume of a gas according to Boyle's law?
Boyle's law states that the pressure of a gas is inversely proportional to the volume of the gas at constant temperature. This means that as the volume of a gas decreases, the pressure increases, and vice versa. Mathematically, this relationship is described by the equation P1V1 = P2V2, where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume, respectively.
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 are some examples of Boyle's and Charles' law problems and how can they be solved?
Examples of Boyle's law problems include calculating the final volume or pressure of a gas when the initial volume or pressure is changed. Charles' law problems involve determining the final temperature or volume of a gas when the initial temperature or volume is altered. These problems can be solved using the respective formulas for Boyle's and Charles' laws, which involve the relationships between pressure and volume, and temperature and volume, respectively.
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.
What if gas is in a sealed container has a pressure of 50 k pa at 300 k what will the pressure be if the temperature rises 360 k?
60kpa
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 effects does temperature have on pressure in a closed container?
Well the temperature of a gas in a container is directly proportional to the pressure of the gas & according to the kinetic theory of gases (viewing gases as made of particles which are in constant random motion) the change in pressure with respect to temperature is given by 2mvx where m is mass and vx the x-coordinate of the initial velocity of the particle. (looking at it as the molecules are colliding with the walls of the container along an axis, x in this case). this proportionality is the basis (implicitly) of Charles's law, Gay-Lussac's law and Boyle's law.
Which container contains water with lower initial temperature?
You think probable to a Dewar container.
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.
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.
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?
No, it is not possible for the balloon to naturally expand four times its initial volume while the temperature remains constant. According to Boyle's Law, at constant temperature, the pressure and volume of a gas are inversely proportional. Since the atmospheric pressure remains constant, the balloon's pressure of 200.0kPa would need to increase to expand, which cannot happen at constant temperature.
If the gas is compressed to a volume of 7.600mL the temperature will rise to 26.00C and resulting pressure will be?
To determine the resulting pressure when the gas is compressed to a volume of 7.600 mL at a temperature of 26.00°C, we can use the ideal gas law (PV = nRT) or apply the combined gas law if we have initial conditions. Without specific initial conditions or the amount of gas, we cannot calculate the exact pressure. However, if you provide the initial pressure, volume, and temperature, we can find the new pressure using the combined gas law.
How valid is the assumption that the initial temperature of the steam is 100 degrees celsius?
The assumption that the initial temperature of steam is 100 degrees Celsius is generally valid when referring to saturated steam at atmospheric pressure. However, it's important to consider that the temperature of steam can vary depending on the pressure or if it is superheated. Additional information or measurements may be needed to confirm the exact initial temperature of the steam in a specific scenario.
