At the same temperature and pressure, 1.0 liter of CO(g) and 1.0 liter of CO2(g) have A. equal masses and the same number of molecules B. different masses and a
Chemistry
annc2apridanza
Question
At the same temperature and pressure, 1.0 liter of CO(g) and 1.0 liter of CO2(g) have
A. equal masses and the same number of molecules
B. different masses and a different number of molecules
C. equal volumes and the same number of molecules
D. different volumes and a different number of molecules
A. equal masses and the same number of molecules
B. different masses and a different number of molecules
C. equal volumes and the same number of molecules
D. different volumes and a different number of molecules
2 Answer

1. User Answers tomvancura
C is the correct answer. All gases have the same volume under the same conditions.. This is just their nature. And one liter of a gas has the same number of molecules of another gas 
2. User Answers Ishankahps
Answer is C  equal volumes and the same number of molecules.
Explanation;
Let's assume that CO and CO₂ are ideal gases. Then we can use ideal gas law, PV = nRT
Where, P is the pressure of the gas (Pa), V is the volume of the gas (m³), n is the number of moles of gas (mol), R is the universal gas constant ( 8.314 J mol⁻¹ K⁻¹) and T is temperature in Kelvin.
The temperature and the pressure of the both gases are same. Volume is also same as 1.0 L. R is a constant. So according to the formula, both gases have same number of moles. According to the Avogadro's constant, 1 mole has 6.022 x 10²³ particles.
number of molecules = Avogadro's constant x number of moles.
Hence, under the same conditions both gases have same number of molecules.