Physics

0.75 mol of argon gas is admitted to an evacuated 40 cm^{3} container at 40 C. The gas then undergoes an isochoric heating to a temperature of 500 C.

Before I forgot to write the question...so the question is What is the final pressure of the gas?

* physics - drwls, Friday, December 11, 2009 at 11:07am

What is the question?
I had to look up "isochoric". It means "contant volume". During that heating process, p will increase such that it remains proportional to (absolute) T. The absolute temperature increases by a factor 773/313 = 2.47. Pressure increases by the same factor. They do not tell you the initial pressure, but you can get the pressure using

P = nRT/V

where R = 82.06 cm^3*atm/mole K

Po = 0.75*82.06*313/40 = 482 atm

I have to get the answer in kPa so I got 4.883865e^4 kPa...but it is wrong

  1. 👍 0
  2. 👎 0
  3. 👁 176
  1. ok...now tired
    P=(0.75)*(8.31)*(773-313)/(4*10^-5)=106373
    106373/1000=106.37kPa..still wrong

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chem

    The solubility of argon in water at 25°C is 0.0150 mol/L. What is the Henry's Law constant for argon if the partial pressure of argon in air is 0.00934 atm?

    asked by Esra on December 30, 2017
  2. Chem

    A flexible container at an initial volume of 5.12 L contains 7.51 mol of gas. More gas is then added to the container until it reaches a final volume of 18.3 L. Assuming the pressure and temperature of the gas remain constant,

    asked by wendy on December 10, 2014
  3. physics

    A container holds 2.2 mol of gas. The total average kinetic energy of the gas molecules in the container is equal to the kinetic energy of a 7.7x10-3 kg bullet with a speed of 650 m/s. What is the Kelvin temperature of the gas?

    asked by natasha on January 28, 2013
  4. Chemistry

    A mixture of nitrogen gas and hydrogen gas reacts in a closed container to form ammonia gas. The reaction ceases before either reactant is completely consumed. At this stage the container has 3.0 mol each of all three gases;

    asked by megs on June 30, 2013
  5. Chem hw!

    1. What pressure would be needed to compress 25.1 mL of hydrogen at 1.01 atm to 25% of its original volume? 2. If the pressure on a 1.04-L sample of gas is doubled at constant temperature, what will be the new volume of the gas?

    asked by Teisha on March 11, 2010
  1. Chemistry

    Ideal gas law question A 4.0 liter container has two gases inside, neon and argon. It is known that at 18 °C, the total pressure of the combined gases is 0.850 atm. If it is known that there are 0.100 moles of neon in the

    asked by Thao on April 25, 2011
  2. sciencee

    1. What pressure would be needed to compress 25.1 mL of hydrogen at 1.01 atm to 25% of its original volume? 2. If the pressure on a 1.04-L sample of gas is doubled at constant temperature, what will be the new volume of the gas?

    asked by Teisha on March 9, 2010
  3. Chemistry

    A 1.30-L sample of argon gas is at 1.02 atm and 21.5 degrees Celsius. a. what mass of argon is in the container. b. If the temperature is raised to 500 degrees celsius while the volume remains constant, calculate the new pressure,

    asked by Dee on November 9, 2012
  4. Physics

    0.75 mol of argon gas is admitted to an evacuated 40 cm^{3} container at 40 C. The gas then undergoes an isochoric heating to a temperature of 500 C. What is the final pressure of the gas?(answer in kPa)

    asked by Ana on December 10, 2009
  5. Chemistry (partial pressure)

    A mixture consists of 3.2 grams of CH4 gas and 1.2 grams of H2 in a steel container. The pressure inside the container is 6.0 atm. The molecular mass of CH4 is 16 g/mol, and the molecular mass of H2 gas is 2 g/mol. What is the

    asked by Summer on March 14, 2018
  6. Chemistry-w/addition

    At elevated temperatures, SbCl5 gas decomposes into SbCl3 gas and Cl2 gas as shown by the following equation: SbCl5(g) SbCl3(g) + Cl2(g) (a) An 59.8 gram sample of SbCl5 (molecular weight 299.0) is placed in an evacuated 15.0

    asked by Fred on January 15, 2011

You can view more similar questions or ask a new question.