If 50.0 L of hydrogen chloride gas reacts with 10.0 L of oxygen gas, what is the volume of chl

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

If $50.0 \mathrm{~L}$ of hydrogen chloride gas reacts with $10.0 \mathrm{~L}$ of oxygen gas, what is the volume of chlorine gas produced? Assume all gases are at the same temperature and pressure. $$\mathrm{HCl}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{Cl}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)$$

If $50.0 \mathrm{~L}$ of hydrogen chloride gas reacts with $10.0 \mathrm{~L}$ of oxygen gas, what is the volume of chlorine gas produced? Assume all gases are at the same temperature and pressure.
$$\mathrm{HCl}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{Cl}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)$$

Key Concepts

Balanced Chemical Equations

A balanced chemical equation ensures that the number of atoms of each element is equal on both sides of the reaction. It lays the foundation for establishing correct mole ratios among reactants and products, which is essential for accurate stoichiometric calculations.

Stoichiometry

Stoichiometry involves using the mole ratios provided by the balanced chemical equation to relate the quantities of reactants and products. It allows the prediction of how much product is formed from given amounts of reactants under specified conditions.

Limiting Reactant

The limiting reactant is the substance in a chemical reaction that is completely consumed first, thereby determining the maximum amount of product that can be formed. Identification of the limiting reactant is crucial because it limits the extent of the reaction regardless of the excess of other reactants.

Avogadro's Law

Avogadro's Law states that equal volumes of all gases at the same temperature and pressure contain an equal number of moles. This principle enables the direct use of volume ratios in stoichiometric calculations when the reacting gases are under identical conditions.

Transcript

00:01 In this question, hydrogen chloride gas reacts with oxygen gas in order to produce chlorine gas, as well as some water in gas form.

00:12 Now, the question states that all gases are at the same temperature and pressure.

00:18 And this tells us that specific volume ratios will be equal to corresponding mole ratios.

00:24 So we will use these ratios in order to solve this question.

00:30 We can do that, we need to balance the equation.

00:35 So if we have a look here at the right -hand side, there's one oxygen on the right -hand side and there's two on the left -hand side.

00:47 So let's put two in front of the water.

00:51 And therefore, we need to increase the number of hydrogen on the left -hand side.

00:57 It needs to be four, same as on the right -hand side.

01:00 And then we need two in front of the chlorine gas.

01:08 All right.

01:08 So now the reaction equation is balanced and we can go ahead with our calculations.

01:15 There will be a limiting reactant that we need to identify here.

01:21 They provide the volumes of both reactants in this question.

01:27 So we can't just take any of these in order to calculate the volume of chlorine.

01:31 Gas that forms.

01:32 We need to figure out which one is limiting the amount of product that can form first.

01:39 In order to do so, we will calculate the volume of chlorine gas produced by starting off with 50 litres of hcl and then compare that volume with the volume of chlorine gas that forms when starting off with 10 litres of oxygen gas.

01:57 Right, so let's do the first calculation.

02:00 For the first calculation, we use the volume ratio of a chlorine gas over the volume of hydrogen chloride gas, and this is equal to 2 over 4...

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