A sample of argon gas has a volume of 735 mL at a pressure of 1.20 atm and a temp of 112 degrees Celsius. What is the final volume of the gas, in milliliters, when the pressure and temp of the gas is changed to

A.) 658 mmHg and 281K?
B.) 0.55 atm and 75 degrees C
C.)15. 4 atm and -15 degrees C

Please help !

Use (P1V1/T1) = (P2V2/T2)

P is in atm, T in kelvin, V will be in L and convert to mL. R is 0.08205 L*atm/mol*k
For a you will need to convert mm Hg to atm. atm = 658/760 = ?
For b you have atm, you will need to convert C to K. 273 + C = K
For c same conversions as b.
Post your work if you would like for me to check your answers.

658mmhg and 281 k

for a i got 743

To solve this problem, we can use the ideal gas law equation, which relates the pressure, volume, and temperature of a gas:

PV = nRT

where:
P is the pressure of the gas
V is the volume of the gas
n is the number of moles of the gas
R is the ideal gas constant
T is the temperature of the gas in kelvin

First, we need to convert the given temperature in degrees Celsius to Kelvin by adding 273.15 to the Celsius temperature.

Given:
Initial volume (V1) = 735 mL
Initial pressure (P1) = 1.20 atm
Initial temperature (T1) = 112 degrees Celsius = (112 + 273.15) K

To find the final volume (V2), we need to calculate the number of moles of the gas using the ideal gas law equation. Then we can rearrange the formula to solve for V2:

V2 = (nRT2) / P2

where:
T2 is the final temperature in Kelvin
P2 is the final pressure

A.) For the first case, the pressure is given in mmHg, so we need to convert it to atm by dividing it by 760 mmHg/atm. The temperature is given in degrees Celsius, so we convert it to Kelvin as mentioned earlier.

Final pressure (P2) = 658 mmHg / 760 mmHg/atm = 0.864 atm
Final temperature (T2) = 281 degrees Celsius = (281 + 273.15) K

Now we can plug these values into the equation to calculate the final volume (V2):

V2 = (nRT2) / P2

To find 'n', we can use the equation n = PV / RT, where P and V are the initial pressure and volume, respectively.

n = (P1 * V1) / (R * T1)

Here, R is the ideal gas constant, which is 0.0821 L.atm/mol.K.

Plugging in the values, we have:
n = (1.20 atm * 735 mL) / (0.0821 L.atm/mol.K * (112 + 273.15) K)

Solving this, we get the value of 'n'.

Then we can calculate the final volume V2 using the equation:
V2 = (n * R * T2) / P2

Substitute the calculated value of 'n', R, T2, and P2 into the equation to find V2.

B.) To solve for the second case, follow the same steps by converting the given temperature to Kelvin and using the given pressure directly.

Final pressure (P2) = 0.55 atm
Final temperature (T2) = 75 degrees Celsius = (75 + 273.15) K

Use the ideal gas law equation to find the final volume (V2) as explained in case A.

C.) For the third case, follow the same steps with the given pressure and temperature.

Final pressure (P2) = 15.4 atm
Final temperature (T2) = -15 degrees Celsius = (-15 + 273.15) K

Use the ideal gas law equation to find the final volume (V2) as explained before.

By following these steps and substituting the given values into the equations, you can find the final volume of the argon gas in each case.