Ok this is a chemistry question about the ideal gas law?

Question

the formula is PV=nRT where P- is pressure (atmospheric) V- volume in liters n- number of moles R- gas constant and T- is temperature in kelvin.. question number 1 . calculate the volume of 1.88 mol of an ideal gas at 55 degrees C and 1.08 atmosphere
question 2. Calculate the pressure of 15.7 mol of an ideal gas in a volume of 268L at 17 degrees C. I dont know how to convert Celcius to kelvin and how to i find out what the ideal gas is... any answers????

ok i got the kelvin thing now but what i am still puzzled about is how to find the gas constant... I know how to plug it in and all that but i need to know what the gas constant is in order for my formula to be complete

thanx a million i managed to solve this thing

Answer 1

First, you have to understand what an ideal gas is. Read your book.

Second, derive your ideal gas equation to get V for Q1, and P for Q2. This is easy.

To convert Celsius to Kelvin, add 273 to the temperature you have in Celsius. So, if you have 17C, its value in Kelvin is 290K.

For the gas constant,
R = 0.08206 L*atm / mol*K

Plug your values to the ideal gas equation. Good luck!

Answer 2

You need R = 0.0820574587 L · atm · K-1 · mol-1
and Kelvin = Celsius + 273.15.
The assumption of ideal gas is irrespective of what the gas is chemically. All you need at this point is to plug the values into the formula and solve:

(1.08 atm)V = (1.88 mol)(0.0820574587 Latm/(°Kmol))(55 + 273.15)°K

P(268 L) = (15.7 mol)(0.0820574587 Latm/(°Kmol))(17 + 273.15)°K

Answer 3

To convert to kelvin, add 273 to your celsius value.
For the first question, just plug in all your values and solve for V.
For question 2, do the same as you did in question 1, but solve for P.

Answer 4

Celcius to Kelvin.....add 273 to celcius.....you do the rest.

Answer 5

Dig under the ground then put your head in it