Question

You have a 5-liter container with 2.00 x 10^23 molecules of ammonia gas (NH3) at STP. How many molecules of argon gas (Ar) are in an identical container at the same temperature and pressure?A. 6.02 x 10^24 moleculesB. 1.30 x 10^24 moleculesC. 2.00 x 10^23 moleculesD. 6.02 x 10^23 molecules

Answer 1

Answer:

C. $2.00\times 10^{23}$ molecules

Explanation:

Since, the temperature, pressure and volume conditions are same, the molecules of ammonia gas must be equal to the molecules of the argon according to the ideal gas equation which is shown below as:-

$PV=nRT$

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 0.0821 L.atm/K.mol

Thus, both will have same moles and same number of molecules.

Thus, molecules of argon = $2.00\times 10^{23}$ molecules