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

Answer 1

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

Answer 2

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.