If 10.0 L of hydrogen chloride gas reacts with 50.0 L of oxygen gas according to the equation

If 10.0 L of hydrogen chloride gas reacts with 50.0 L of...

If $10.0 \mathrm{~L}$ of hydrogen chloride gas reacts with $50.0 \mathrm{~L}$ of oxygen gas according to the equation in Exercise $73,$ what is the volume of chlorine gas produced? Assume all gases are at the same temperature and pressure.

Key Concepts

Avogadro's Law

Avogadro's Law states that equal volumes of all gases at the same temperature and pressure contain equal numbers of molecules. This concept is crucial in gas stoichiometry because it allows the volumes of reacting gases to be directly used in the same ratios as the coefficients in a balanced chemical equation, eliminating the need for conversion to moles when temperature and pressure are constant.

Chemical Stoichiometry

Chemical stoichiometry involves the calculation of reactants and products in chemical reactions by using the mole ratios derived from the balanced chemical equation. In gas reactions at constant temperature and pressure, these mole ratios are equivalent to volume ratios, which simplifies the analysis of how much of a product is formed based on the volumes of reactants available.

Limiting Reactant

The concept of a limiting reactant is important in reactions because it determines the maximum amount of product that can be formed. Even when dealing with gases, identifying which reactant is present in the lesser amount relative to its required stoichiometric coefficient prevents overestimating the yield, ensuring that calculations for product volume are based on the reactant that runs out first.

Transcript

00:01 In this question, we need to make use of the reaction equation that we've used in the previous question.

00:07 So i've copied the balanced equation onto this page.

00:14 We also need to realize that it's the same as with the previous question.

00:20 We can assume that all gases are at the same temperature and pressure, which means that specific volume ratios will be equal to corresponding mole ratios.

00:30 And then another point that we need to take into account here is that the volume of both reactants, the volumes of both reactants are provided.

00:41 So we therefore need to look out for limiting reactant.

00:47 We will determine the limiting reactant by comparing the volume of chlorine gas produced when starting off with 10 litres of hydrogen.

01:00 Chlorine acid or hydrogen chloride gas with the volume of chlorine gas that forms when starting off with 50 liters of oxygen gas.

01:14 Right.

01:14 So let's do the first calculation where we calculate the volume of chlorine gas from 10 liters of hcl.

01:24 So we need to use the mole ratio here.

01:30 The mole ratio of chlorine to hcl is 2 to 4, which is equal to a half.

01:40 We can therefore say that the volume of chlorine gas is equal to a half times the volume of the hydrogen chloride gas, and that's equal to a half times 10 litres, 10 .0 liters, which is equal to 5 .00 liters.

02:01 Now we will do the same type of calculation for when starting off with 50 litres of oxygen...

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