Consider the following gas phase reaction: H2(g)+Cl2(g) →2 HCl(g) . If 8.36 liters of Cl2(g) gas

step 1 Hi there. This is a gas stoichiometry problem. And to solve any stoichiometry problems, we need

Consider the following gas phase reaction: H2(g)+Cl2(g) →2...

Consider the following gas phase reaction: $\mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(\mathrm{g})$ $\rightarrow 2 \mathrm{HCl}(\mathrm{g}) .$ If 8.36 liters of $\mathrm{Cl}_{2}(\mathrm{g})$ gas at $113^{\circ} \mathrm{C}$ and 0.693 atm is used, what volume of HCl(g) gas will be formed if it is collected at $64^{\circ} \mathrm{C}$ and 0,355 atm?

Consider the following gas phase reaction: $\mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(\mathrm{g})$ $\rightarrow 2 \mathrm{HCl}(\mathrm{g}) .$ If 8.36 liters of $\mathrm{Cl}_{2}(\mathrm{g})$ gas at $113^{\circ} \mathrm{C}$ and 0.693 atm is
used, what volume of HCl(g) gas will be formed if it is collected at $64^{\circ} \mathrm{C}$ and 0,355 atm?

Key Concepts

Combined Gas Law

The Combined Gas Law integrates the relationships between pressure, volume, and temperature for a fixed amount of gas. It provides a single equation to calculate the new conditions of a gas when multiple state variables change simultaneously.

Temperature and Pressure Corrections

This concept involves adjusting gas volumes when conditions such as temperature and pressure change. It requires converting temperatures to an absolute scale and applying rigorous relationships to predict how changes in these variables affect the gas volume.

Ideal Gas Law

The Ideal Gas Law, expressed as PV = nRT, relates the pressure, volume, and temperature of a gas to the number of moles present. It is crucial for converting between these variables under the assumption that the gas behaves ideally.

Stoichiometry

Stoichiometry deals with the quantitative relationships between reactants and products in a chemical reaction. It allows for the calculation of the amounts of substances involved based on the balanced equation, which sets the relative number of moles of each reactant and product.

Transcript

00:01 Hi there.

00:02 This is a gas stoichiometry problem.

00:04 And to solve any stoichiometry problems, we need a balanced equation.

00:08 That is the first thing i want to grab out of this problem is the balanced equation that we are provided.

00:14 Hydrogen gas plus chlorine gas is producing 2hcl, hydrochloric or hydrogen chloride gas.

00:27 All right.

00:28 So all of these are gases.

00:29 We are given 8 .36 liters.

00:35 Of cl2, and we want to know how many liters of hcl we can make.

00:41 This problem would be very quick.

00:43 It would just be one step if both of our gases were at the same temperature and pressure.

00:47 However, they are not.

00:49 The chlorine is starting at a different temperature and pressure than the hcl is ending at.

00:55 Because of that, we are going to have to do a little extra work here.

01:00 First, let's list out all of the things that we know.

01:03 The chlorine is at 113 degrees celsius.

01:06 I'm going to convert that to kelvin by adding 273, and i get 386 kelvin.

01:15 We're also told that the pressure of the chlorine is 0 .693 atmospheres.

01:25 The hcl is at 64 degrees celsius, converting that to kelvin by adding 273.

01:36 We get 337 kelvin.

01:41 The pressure of the hcl, or the pressure that the hcl is collected at is 0 .355 atmospheres.

01:54 Since these two gases are at different temperatures and pressure, i need to adjust the volume of chlorine to the temperature and pressure that the hcl is going to be collected at.

02:08 So i need to adjust these and then i can use stoichiometry to solve the problem.

02:14 The way that i'm going to adjust these is by using the combined gas law...

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