Gaseous chlorine dioxide, ClO2, is used to bleach flour and in water treatment. It is produced b

step 1 Hi there. This problem is a gas stoichiometry problem. So just like in any stoichiometry problem

Gaseous chlorine dioxide, ClO2, is used to bleach flour and...

Gaseous chlorine dioxide, $\mathrm{ClO}_{2},$ is used to bleach flour and in water treatment. It is produced by the reaction of chlorine with sodium chlorite: $\mathrm{Cl}_{2}+2 \mathrm{NaClO}_{2} \rightarrow 2 \mathrm{ClO}_{2}+2 \mathrm{NaCl}$. How many liters of $\mathrm{ClO}_{2}$, measured at 0.961 atm and $31^{\circ} \mathrm{C},$ will be produced by $283 \mathrm{L} \mathrm{Cl}_{2}$ at 2.92 atm and $21^{\circ} \mathrm{C} ?$

Gaseous chlorine dioxide, $\mathrm{ClO}_{2},$ is used to bleach flour and in water treatment. It is produced by the reaction of chlorine with sodium chlorite: $\mathrm{Cl}_{2}+2 \mathrm{NaClO}_{2} \rightarrow 2 \mathrm{ClO}_{2}+2 \mathrm{NaCl}$. How many
liters of $\mathrm{ClO}_{2}$, measured at 0.961 atm and $31^{\circ} \mathrm{C},$ will be produced by $283 \mathrm{L} \mathrm{Cl}_{2}$ at 2.92 atm and $21^{\circ} \mathrm{C} ?$

Key Concepts

Gas Law Corrections

Gas law corrections, including the use of the Ideal Gas Law and the Combined Gas Law, enable the adjustment of measurements of gas volumes when the gases are at different pressures and temperatures. This is crucial for accurately determining the amount of gas produced or consumed when conditions are not standard.

Stoichiometry

Stoichiometry involves using the balanced chemical equation to determine the quantitative relationships between reactants and products. It allows for calculating the moles or volumes of products that will be formed from given amounts of reactants by using the mole ratios provided in the balanced equation.

Ideal Gas Law

The Ideal Gas Law, expressed as PV = nRT, is a fundamental relation that describes the behavior of gases. It relates a gas's pressure, volume, temperature, and number of moles, enabling the conversion and comparison of gas quantities under varying conditions of temperature and pressure.

Transcript

00:01 Hi there.

00:02 This problem is a gas stoichiometry problem.

00:06 So just like in any stoichiometry problem, we know we are going to need a balanced equation.

00:11 So i am going to grab the balanced equation here from the problem.

00:17 It's chlorine gas plus 2 naclo2 produces 2 c -l -2, which is a gas, plus 2 nacl .cl .l .2, which is a gas, plus 2 nacl.

00:44 Is our balanced equation, and we are given 283 liters of chlorine gas, and we are trying to figure out how many liters of the clo2 we can make when we start with that 283 liters of chlorine gas.

01:06 The thing about this problem is, however, is that these two gases are not at the same pressure.

01:11 The chlorine gas begins at one pressure, and then the clo2 is produced at a different temperature and pressure.

01:21 So we will need to take those into account.

01:24 Since they are not the same temperature and pressure, we cannot just do a straight gas stoichiometry on this problem.

01:31 Let's look at the other information that we have here.

01:34 We have 2 .92 atmospheres is what this gas is at at the beginning, and 21 degrees celsius.

01:44 I'm just going to go ahead and convert that to kelvin right away because i know it's a gas law problem and temperature must be in kelvin for gas law problems.

01:58 The cl02 is collected at a pressure of .961 atmospheres and a temperature of 31 degrees celsius.

02:14 Converting that to kelvin, we get 304 kelvin.

02:20 What we need to do, before we can use the balanced equation to do the stoichiometry to get from chlorine gas to the clo2, what we need to do is calculate how many liters of chlorine gas we would have under the conditions of the product, clo2.

02:46 To do that, i'm going to have to use the combined gas law.

02:51 In other words, p1v1 over t1 equals p1.

02:58 V2 over t2, where the initial conditions are the conditions that the chlorine is starting at, and the new conditions are those that the product is at...

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