Answer:
D) 2L of H2 & 2L of Cl2
Explanation:
As according to universal gas law,
PV=nRT
V=nRT/P
For STP condition, T=273.15K, P=1atm n= 1mole
R=0.0819 L atm / mol K
V= 1*0.082*273.15/1 = 22.4 L
So 1 mole of gas at STP has 22.4L of volume
we know, No. of molecules= no of moles* Avogadro's Number
A) 1L of CO & 0.5L of N2
1L of CO:
Number of moles in 22.4L of CO = 1
Number of moles in 1L of CO = 1/22.4=0.045 moles
Number of molecules in 1L of CO= 0.045*Avogadro's Number
0.5L of N2
Number of moles in 22.4L of N2= 1
Number of moles in 0.5L of N2= 1/22.4=0.022 moles
Number of molecules in 0.5L of N2= 0.022*Avogadro's Number
So both are not equal, A is not our answer
B) 2L of CO & 0.5L of NH3
1L of CO:
Number of moles in 22.4L of CO = 1
Number of moles in 2L of CO = 2/22.4=0.089 moles
Number of molecules in 2L of CO= 0.089*Avogadro's Number
0.5L of NH3
Number of moles in 22.4L of NH3= 1
Number of moles in 0.5L of NH3= 1/22.4=0.022 moles
Number of molecules in 0.5L of N2= 0.022*Avogadro's Number
So both are not equal, B is not our answer
C) 1L of H2 & 2L of Cl2
1L of H2:
Number of moles in 22.4L of H2 = 1
Number of moles in 1L of H2 = 1/22.4=0.045 moles
Number of molecules in 1L of H2= 0.045*Avogadro's Number
2L of Cl2
Number of moles in 22.4L of Cl2= 1
Number of moles in 2L of Cl2= 1/22.4=0.089 moles
Number of molecules in 2L of Cl2= 0.089*Avogadro's Number
So both are not equal, C is not our answer
D) 2L of H2 & 2L of Cl2
2L of H2:
Number of moles in 22.4L of H2 = 1
Number of moles in 1L of H2 = 2/22.4=0.045 moles
Number of molecules in 2L of H2= 0.089*Avogadro's Number
2L of Cl2
Number of moles in 22.4L of Cl2= 1
Number of moles in 2L of Cl2= 1/22.4=0.089 moles
Number of molecules in 2L of Cl2= 0.089*Avogadro's Number
So both are not equal, D is our answer
