Question

If 6.5 grams of CO react, how many litres of $C{{O}_{2}}$ are produced?

Answer 1

Hint: Find the Number of moles of carbon monoxide and then find the volume of carbon dioxide produced by substituting it in the ideal gas equation.

Complete answer:
In order to answer the question, we need to know about moles and molar mass. Now, matter is made up of atoms, and as matter has mass, then the atoms should have an individual mass. Molar mass of an element or compound is the mass which houses $6\times {{10}^{23}}$ particles. For, example, the hydrogen molecule has a molar mass of 2 grams. This means 2 grams of hydrogen contains $6\times {{10}^{23}}$atoms, and this number is also called the Avogadro’s number.
Number of moles of an element or a compound is the ratio of its given mass taken by the user, to its molar mass. More is the number of moles, more is the concentration of the substance. Now, let us come to the question. In order to analyse the situation, we will write down the equation for the conversion of carbon monoxide to carbon dioxide:
\[CO(g)+\dfrac{1}{2}{{O}_{2}}\to C{{O}_{2}}(g)\]
All of the reactants and the products are gaseous, which means that the ideal gas equation can be applied to them. Let us first calculate the number of moles of carbon monoxide; the number of moles is given by the formula $no\,of\,mole=\dfrac{given\,mass}{molar\,mass}$, so the number of moles is $mol{{e}_{CO}}=\dfrac{6.5}{28}=0.23$. Assuming the reaction is taking place at conditions of standard temperature and pressure, we can find the volume using the ideal gas equation which is:
\[\begin{align}
  & PV=nRT \\
 & \Rightarrow V=\dfrac{nRT}{P} \\
 & \Rightarrow V=\dfrac{0.23\times 0.0821\times 298}{1}\cong 160L \\
\end{align}\]
So 6.5 grams of carbon monoxide, when reacted with oxygen , gives out 160 litres of carbon dioxide.

Note:
It is to be noted that the volume of the carbon dioxide produced is directly proportional to the number of moles of carbon monoxide taken.