How many molecules of O2 are present in a 3.90L flask at a temperature of 273K and a pressure of 1.00atm?
Select the correct answer below:
A) 1.05×10^23 molecules
B) 1.74×10^23 molecules
C) 3.74×10^24 molecules
D) 9.60×10^22 molecules
Answer : option(A) is the correct option
Given : V = 3.9 L , T = 273 K , P = 1atm
And we know R (gas constant ) = 0.0821 L atm mol-1 K-1
Using ideal gas equation : PV = n * R * T
Where n = no. of moles of O2 gas
n= P * V / (R* T) = 1 * 3.9 /(0.0821 * 273 ) = 0.174 moles
As 1 mole of O2 contain= 6.022 * 1023 molecules
So, 0.174 mole of O2 contain = 0.174 * 6.022 * 1023
= 1.05 * 1023 molecules
Which is option (A)
How many molecules of O2 are present in a 3.90L flask at a temperature of 273K...
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