Consider the following representation of a gaseous chemical reaction. If carried out at constant temperature and pressure how would the volume in the container before the reaction (V_r)compare to that after the reaction (V_p)?

Question

Quizplus · Accepted Answer

According to Avogadro's Law, at constant temperature and pressure, equal volumes of gases contain equal numbers of molecules. The reaction involves the conversion of one molecule of reactant (A) to two molecules of product (B and C). Therefore, for every 2 moles of product (B and C), one mole of reactant (A) is consumed. This means that the number of moles of gas in the container has remained the same before and after the reaction. Since the number of moles of gas is directly proportional to the volume, this means that the initial volume (V_r) must be twice the final volume (V_p) in order to maintain the same number of moles of gas. Therefore, 2V_r = V_p.

Consider the Following Representation of a Gaseous Chemical Reaction