If you are given an ideal gas with pressure (p) = 259,392.00 pa and temperature (t) = 2.00 oc of 1 mole argon gas in a volume of 8.8 dm3 , calculate r to the correct number of significant figures and units under given condition

 R = 0.064 dm³ atm K⁻¹ mol⁻¹

Explanation:

Explanation:

Data Given:

volume of gas V = 8.8 dm³

no. of mole of gas (n) = 1 mole

Pressure P = 259,392.00 Pa  

Convert Pascal (Pa) to atm (atmospheric pressure)

As

101,325 Pascals = 1 atm

So,

259,392.00 Pa  = 2 atm

Then Pressure (P) = 2 atm

Temperature T = 2.00 °C  

change the temperature from °C to K

As  to convert °C to K the below formula used

                   0°C + 273.15 = 273.15K

So, for 2 °C

                    2°C  + 273.15 =  275.15 K

So,

Temperature T  = 275.15 K

ideal gas constant = ?

formula used for Ideal gases

                            PV = nRT

as we have to find R of the gas:

we will rearrange the ideal gas equation as below:

R = PV / nT (1)

Put value in equation (1)

                 R = 2atm x 8.8 dm³ / 1 mole x 275.15 K

                  R = 17.6 atm. dm³ / 275.15 mol. K

                  R = 0.064 dm³ atm K⁻¹ mol⁻¹

So the value of R is 0.064 dm³ atm K⁻¹ mol⁻¹

and the unit of R (ideal gas constant) is dm³ atm K⁻¹ mol⁻¹

the answer is a! (2.9 x 10^-18 j) hope i could someone. : )