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The ideal gas law, (PV = nRT), can be used here. The initial pressure is proportional to the initial number of moles, and the final pressure is proportional to the total number of moles. Therefore, the ratio of final pressure to initial pressure is the ratio of the total number of moles of gas at the final conditions to the number of moles initially in the container.
What else can I help you with?
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.
A gas with a volume of 4.00 L at a pressure of 205 kPa is allowed to expand to a volume of 12.0 L. What is the pressure in the container if the temperature remains constant?
Using the ideal gas law (PV = nRT) and assuming the number of moles and temperature remain constant, the initial and final pressures can be related by P1V1 = P2V2. Plugging in the values, the final pressure in the container after expansion to 12.0 L is 68.3 kPa.
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.
What is the temperature of a soda if you put it in ice for 30 mins?
The temperature of the soda will decrease due to the ice's lower temperature, but it will not reach the same temperature as the ice. The rate of cooling will depend on various factors such as the initial temperature of the soda, the amount of ice, and the thermal conductivity of the container.
A tire has pressure of 325 kpa at 10c if the temperature of the tire rises to 50c and the volume remains constantwhat is new pressure?
Using the ideal gas law, we can calculate the new pressure using the formula P1/T1 = P2/T2. Plugging in the initial pressure (325 kPa), initial temperature (10°C), and new temperature (50°C), we can solve for the new pressure. The new pressure would be approximately 541 kPa.
If pressure of gas in container is psi what is the pressure if volume of container is halved?
According to Boyle's Law, the pressure of a gas is inversely proportional to its volume when temperature is held constant. If the volume of a container is halved, the pressure will double. Therefore, if the initial pressure is ( P ) psi, the new pressure will be ( 2P ) psi after halving the volume.
What is the correct relationship to use in finding the final pressure of a sample of gas after it has been heated in a rigid container?
To find the final pressure of a gas sample after it has been heated in a rigid container, you can use the ideal gas law, ( P_1/T_1 = P_2/T_2 ). Since the volume is constant in a rigid container, this equation relates the initial and final pressures (P1 and P2) to the initial and final temperatures (T1 and T2) in Kelvin. Thus, by measuring the initial pressure and temperature and knowing the final temperature, you can calculate the final pressure.
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.
A gas with a volume of 4.00 L at a pressure of 205 kPa is allowed to expand to a volume of 12.0 L. What is the pressure in the container if the temperature remains constant?
Using the ideal gas law (PV = nRT) and assuming the number of moles and temperature remain constant, the initial and final pressures can be related by P1V1 = P2V2. Plugging in the values, the final pressure in the container after expansion to 12.0 L is 68.3 kPa.
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 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
What will be the final temperature of a fixed quantity of air originally at 22 C in a rigid container if its pressure increases from 730 mm Hg to 795 mm Hg?
To determine the final temperature of the air in the rigid container, you would need to know the volume of the container and the gas constant for air. Using the ideal gas law (PV = nRT), you can calculate the initial and final temperatures. Without this information, it is not possible to determine the final temperature of the air in the container accurately.
How do you test the effect of removing heat from a gas that is stored in a sealed container?
To test the effect of removing heat from a gas in a sealed container, you can use a calorimeter or a thermally insulated chamber to monitor temperature changes. Start by measuring the initial temperature and pressure of the gas. Then, apply a cooling method, such as placing the container in an ice bath or using a refrigeration system, and observe changes in pressure and volume. Analyze the data to understand how the gas's behavior relates to temperature reduction, using gas laws (e.g., Charles's Law) for further insight.
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 will its pressure be at W degrees Celsius if the volume does not change?
To determine the pressure at W degrees Celsius with a constant volume, you can use the ideal gas law, where pressure is directly proportional to temperature in Kelvin. Convert W degrees Celsius to Kelvin by adding 273.15, then apply the formula ( P \propto T ). If the initial pressure and temperature are known, you can calculate the new pressure using the ratio of the new temperature to the initial 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?
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.
