Ideal gas law?

Question

Directions (For all problems use the following units: atm, Kelvin, moles and Liters)
What are the units on each of the variables in the ideal gas equation?
PV = nRT
2. If a gas sample has a temperature of 32.5 degrees Celsius, what is the temperature of the gas in Kelvins?
3. What is the volume of 1 mol of an ideal gas at 273 K and 1 atm of pressure?
4. What is the temperaure (in Kelvins) of a sample of an ideal gas if 1.5 moles of the gas occupy a volume of 27 liters at 1.1 atm.
I have some answers but i want to make sure is correct

Answer 1

An ideal gas is defined as one in which all collisions between atoms or molecules are perfectly eleastic and in which there are no intermolecular attractive forces.

An ideal gas can be characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them may be deduced from kinetic theory and is called the
Ideal Gas Law :PV=nRT=NkT
n = number of moles
R = universal gas constant = 8.3145 J/mol K
N = number of molecules
k = Boltzmann constant = 1.38066 x 10-23 J/K = 8.617385 x 10-5 eV/K
k = R/NA
NA = Avogadro's number = 6.0221 x 1023 /mol
The ideal gas law can be viewed as arising from the kinetic pressure of gas molecules colliding with the walls of a container in accordance with Newton's laws. But there is also a statistical element in the determination of the average kinetic energy of those molecules. The temperature is taken to be proportional to this average kinetic energy; this invokes the idea of kinetic temperature. One mole of an ideal gas at STP occupies 22.4 liters.

Answer 2

1.P=pressure--> atm
V=volume--> L
n=number of moles--> moles
R=proportionality constant called the ideal gas constant
R=0.0821 L(atm) / mol(K)
T=temperature in Kelvin--> Kelvin (K)

2.32.5+273= 305.5 Kelvin

3.0.0821*1*273 / 1 = 22.4133 Liters

4. 241 K