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=0·083 J/mol·K

Explanation:

Ideal gas equation is

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× atm

(259,392·00× )×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

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer

a