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
Question
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
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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.