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The volume of a sample of gas initially at 25 C increases from 158 ml to 450 ml What is the final temperature of the sample of gas if the pressure in the container is kept constant?
Wiki User
∙ 12y ago
Using the Ideal Gas Law,
PV = nRT
Solve for n.
n = PV/RT = (101.325 kPa)(0.050 L)/(8.314)(323K) = 0.001886575 mol
Now we know the number of moles of the gas at 50 degrees Celsius (323 Kelvin).
What we need to do now is to solve for the volume at 80 degrees Celsius (353 Kelvin).
V = nRT/P = (0.001886575 mol)(8.314)(353K)/(101.325 kPa) = 0.546 mol
Can you please tell me if this is correct?
Wiki User
∙ 15y ago
Wiki User
∙ 12y agoUsing Charle's law, which involves temperature and volume is V1/T1=V2/T2. To find the final temperature (T2), rewrite the equation to solve for T2.
So T2=T1*V2/V1
Now you can plug everything into the equation and solve. Just don't forget that you need to change 25 degrees Celsius to Kelvin first. (Kelvin = Celsius + 273)
T2=25 + 273 * (450mL/158mL) equals 849 Kelvin. To change back to Celsius,
849-273 = 576 degrees Celsius
Wiki User
∙ 12y agoHey Candi Keller, the answer is 26.3 mL :)
Hey Candi Keller its Connor Hahaha
If it is held in a container, then it will stay as 25.3 L, but the pressure will increase.
Wiki User
∙ 7y agoIn a sealed container the volume remain the same and the pressure increase.
Wiki User
∙ 11y ago26.3 mL
John Gonzalez
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Anonymous
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What would happen to the pressure of a gas sealed container if the volume increases and the temperature stays the same?
If the temperature increases, then the volume of the gases cannot stay the same. The pressure will keep building until it overcomes the integrity of the container its contained in and causes an explosion.
How are the absolute temperature and volume of a gas at constant pressure related?
They're proportional; as temperature increases volume increases.
When the temperature of a gas at constant volume increases it's?
Pressure increases. yup
What is the effect on pressure when the temperature of a gas at constant volume is increased?
Universal Gas Law: P*V/T = a constant, where P = gas pressure [Pa], V = volume [m3], and T = gas temperature [K]. Therefore, when the gas temperature increases, the pressure increases linearly with it, when the volume is constant.
What causes a gas to exert pressure when confined in a container?
Assuming constant amount of gas and temperature, pressure will increase as volume decreases. Conversely, pressure will decrease as volume increases. If you squeeze on a filled balloon, the volume decreases. The pressure of the air on each square inch of the balloon increases, which causes it to eventually pop if the pressure gets too high. Assuming constant amount of gas, a temperature change will already change the volume of the gas. As temperature rises, the gas expands, causing more pressure to be exerted on the balloon. Assuming constant temperature, adding more gas also increases the volume and thus increases the pressure.
Explain why increasing the temperature of a gas in closed rigid container causes the pressure in the container to increase?
Because the pressure increases The real answer is: Charles's Law. He found that if you increase the temperature of a constant pressure the volume increases also.
When the pressure of a gas increases at constant temperature its volume?
Temperature increases as pressure increases.
When solute particles are added to a pure solvent in a closed container at a constant temperature and pressuer the vapor pressure?
it increases
When the temperature of of gas increases at constant pressure its?
As pressure increases, if temperature is constant, the gas will decrease in volume.
When the temperature of a gas increases at constant pressure it's?
As pressure increases, if temperature is constant, the gas will decrease in volume.
When gas in a container expand to twice its volume at constant temperature the gas pressure does what?
The pressure increases. Hopefully, the container is strong enough to withstand the increased pressure. If there is a weakness in the container, gas will escape as a leak.
What would happen to the pressure of a gas sealed container if the volume increases and the temperature stays the same?
If the temperature increases, then the volume of the gases cannot stay the same. The pressure will keep building until it overcomes the integrity of the container its contained in and causes an explosion.
A 4.0 liter container of gas in initially at a pressure of 16 ATM what will the pressure be if the voume is changed to 1 liters at constant temperature?
Use Boyle's Law, applicable for ideal gases at constant temperature, to solve this problem: P1*V1 = P2*V2
When a temperature of a gas at a constant volume increases?
Pressure increases. yup
How are the absolute temperature and volume of a gas at constant pressure related?
They're proportional; as temperature increases volume increases.
How are the volume and pressure of a gas at a constant temperature related?
They're proportional; as temperature increases volume increases.
How are the volume and temperature of a gas at at constant pressure related?
They're proportional; as temperature increases volume increases.
