Question

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.​

Answer 1

R=0·083 J/mol·K

Step-by-step explanation:

Ideal gas equation is

P×V = n×R×T

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 ideal gas constant

T is the temperature of the gas in Kelvin

In case of given problem

Temperature of the gas = 273+2·00=275·00K

P=259,392·00×
`10^(-5)` atm

(259,392·00×
`10^(-5)` )×8·8 = 1×R×275·00

∴R=0·0830 J/mol·K

But according to the rules of significant figures the value of R must be with least precision of all the values of the other parameters from which the value of R is calculated

Here the least precision is in the volume as it contains only 2 significant digits

∴ Value of R must contain 2 significant digits

∴ R=0·083 J/mol·K