Question

Calculate the volume of oxygen at NTP that would be required to convert L of carbon monoxide to carbon dioxide.
A.$5.2$L
B.$2.5$L
C.$3.42$L
D.None of these

Answer 1

The volume of $1$ mole of any gas is called its molar volume and is equal to $22.4\;$ L at standard temperature and pressure (according to the ideal gas law) Molar volume allows conversions to be made between moles and volume of gases at STP.

Complete step by step answer:
The chemical reaction for the equation in the question is :
$CO + \dfrac{1}{2}{O_2} \to C{O_2}$
Final moles of $5$ liters of $CO$ :
If $22.4\;$ liters of $CO$ is $1$ mole
Then $5$ liters of $CO = 1 \times \dfrac{5}{{22.4}} = 0.223\;moles$
The equation for the reaction of the oxidation of $CO$ is
The mole ratio between $CO$ and ${O_2}$​ in the equation is $2:1$
The mole of $5$ litres $CO$ is $0.233$ moles
Since$2:1$ mole ratio is , as seen in the reaction above
We need $\dfrac{{0.233}}{2}$ moles of oxygen
0.112 mol$= 0.112$es of oxygen to react with $CO$
Then $0.112\;moles\; = 0.112 \times 22.4/1 = 2.5\;litre$.
So the correct option is B)

Note: Avogadro’s hypothesis states that equal volumes of all gases at the identical temperature and pressure contain the identical number of particles. A graph of the effect of temperature on the degree of a gas at constant pressure depicts that the amount of a gas is directly proportional to the amount of moles of that gas. this can be called because the Avogadro’s law.
The critical chemical difference is that CO2 contains one atom of carbon and two atoms of oxygen, whilst CO has one carbon and one oxygen atom. carbonic acid gas is non-flammable, whilst CO isn't. greenhouse emission naturally occurs within the atmosphere . However, CO doesn't occur naturally within the atmosphere and might cause health problems even in low concentrations. The density of both gases is additionally different in values.