# Chemistry redox reaction - gases mixing

• Feodalherren
In summary, to react Cl2 with NaI to form IO3- and Cl-, 18.5 mL of gas are needed. This is done by measuring the Cl2 gas at 28.0 °C and 750 torr. The molar mass of NaI is .0030906 mol, so 3 moles of Cl2 are needed for every 1 mol of NaI.
Feodalherren

## Homework Statement

How many milliliters of Cl2 gas, measured at 28.0 °C and 750 torr, are needed to react with 18.5 mL of 0.173 M NaI if the I- is oxidized to IO3- and the Cl2 is reduced to Cl-?

## The Attempt at a Solution

So the molar mass is .0030906 mol NaI. Now I need to find out how many moles of Cl2 are needed to react completely with that.
So I need the balanced chemical equation.

Cl2 + NaI --> IO3- + Cl-

Redox:

2e- + Cl2 --> 2Cl-

NaI --> IO3- + Na+

This is where I get stuck.
I can't balance NaI as a redox reaction because I don't know the charges on that side. How do I balance the second part of the reaction?

Is 3Cl2 + NaI + 3H2O --> IO3- + Na+ + 6H+ + 6Cl-

the correct balanced reaction?

Feodalherren said:
Is 3Cl2 + NaI + 3H2O --> IO3- + Na+ + 6H+ + 6Cl-

the correct balanced reaction?

Technically - yes. But why don't you treat NaI as a dissociated salt (Na++I-), it is dissolved, isn't it?

1 person
Ahh that's what was confusing me. I got the rest of it, thanks.

?

Feodalherren said:
Ahh that's what was confusing me. I got the rest of it, thanks.

what was the solution, I am stumped

So after you have the Redox reaction you have your ratio which is that for every 1 mol of NaI you have 3 moles of Cl2.

You know that you have 18.5 mL of 0.173 M NaI so therefore

.0185 L (.173 mol NaI/L) = moles of NaI.

Now multiply that by three to get the moles of Cl2 because as shown from the balanced chemical equation - you need 3 moles of Cl2 for every 1 mol of NaI.

From there you have

PV=nRT

Make sure to convert P to atm and T to Kelvin. n Is the amount of moles of Cl2 - solve for V. Done.

Edit: oh yeah - convert to mL since that's what the question was asking for.

## 1. What is a redox reaction in chemistry?

A redox reaction, also known as an oxidation-reduction reaction, is a chemical reaction in which there is a transfer of electrons between two substances. One substance is oxidized, or loses electrons, while the other substance is reduced, or gains electrons. This transfer of electrons results in a change in the oxidation states of the substances involved and the formation of new chemical compounds.

## 2. How do you identify a redox reaction?

A redox reaction can be identified by the change in oxidation states of the substances involved. The substance that is oxidized will have a higher oxidation state in the product than in the reactant, while the substance that is reduced will have a lower oxidation state in the product than in the reactant. Additionally, there will be a transfer of electrons from one substance to another, which can be observed through the use of a half-reaction or by tracking the changes in the number of valence electrons.

## 3. What are the different types of redox reactions?

There are two main types of redox reactions: oxidation and reduction. In an oxidation reaction, a substance loses electrons and increases in oxidation state, while in a reduction reaction, a substance gains electrons and decreases in oxidation state. Redox reactions can also be classified as combination, decomposition, displacement, or combustion reactions, depending on the specific chemical process that is occurring.

## 4. How do gases mix during a redox reaction?

Gases can mix during a redox reaction through a process called diffusion. Diffusion is the movement of particles from an area of high concentration to an area of low concentration. In a redox reaction, the gases involved will diffuse and mix together as the reaction progresses, resulting in a homogenous mixture of gases.

## 5. What role do catalysts play in redox reactions involving gases?

Catalysts can play a significant role in redox reactions involving gases. A catalyst is a substance that speeds up the rate of a chemical reaction without being consumed in the process. In redox reactions, a catalyst can provide an alternative pathway for the reaction to occur, lowering the activation energy required for the reaction to take place. This can result in a faster and more efficient reaction, especially in the case of gases mixing during a redox reaction.

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