Consider the reaction: 2 NiO(s) ⟶2 Ni(s)+O2(g) If O2 is collected over water at 40.0^∘ C and a t

Consider the reaction: 2 NiO(s) ⟶2 Ni(s)+O2(g) If O2 is...

Consider the reaction: $$2 \mathrm{NiO}(s) \longrightarrow 2 \mathrm{Ni}(s)+\mathrm{O}_{2}(g)$$ If $\mathrm{O}_{2}$ is collected over water at $40.0^{\circ} \mathrm{C}$ and a total pressure of 745 $\mathrm{mm} \mathrm{Hg},$ what volume of gas is collected for the complete reaction of 24.78 $\mathrm{g}$ of $\mathrm{NiO}^{2}$

Consider the reaction:
$$2 \mathrm{NiO}(s) \longrightarrow 2 \mathrm{Ni}(s)+\mathrm{O}_{2}(g)$$
If $\mathrm{O}_{2}$ is collected over water at $40.0^{\circ} \mathrm{C}$ and a total pressure of 745 $\mathrm{mm} \mathrm{Hg},$ what volume of gas is collected for the complete reaction of 24.78 $\mathrm{g}$ of $\mathrm{NiO}^{2}$

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Key Concepts

Gas Collection Over Water

Collecting gases over water is a common technique that requires accounting for water vapor present in the collected gas. It is important to correct for water vapor in order to accurately determine the amount or volume of the gas being measured.

Vapor Pressure Correction

When gases are collected over water, the total measured pressure is a combination of the gas pressure and the water vapor pressure. By subtracting the known vapor pressure of water at the collection temperature from the total pressure, one obtains the partial pressure of the collected gas, which is then used in further calculations.

Ideal Gas Law

The Ideal Gas Law, expressed as PV = nRT, relates the pressure (P), volume (V), number of moles (n), the ideal gas constant (R), and temperature (T) of a gas. This law is crucial for calculating the volume of a gas under specified conditions of temperature and pressure.

Stoichiometry

Stoichiometry involves using the balanced chemical equation to relate the quantities of reactants and products through their molar ratios. It allows one to determine how many moles of a product are formed from a given amount of a reactant, using the compound's molar mass as a conversion factor.

Transcript

00:01 All right, so in this problem, we are dissolving nickel oxide over water to produce oxygen gas.

00:08 And we are asked to determine how much oxygen is produced in liters from the complete reaction of 24 .78 grams of nickel oxide.

00:16 All right, so first thing first, i'm going to notice that i'm going to be using the ideal gas law.

00:25 So pv equals nrt.

00:28 And i'm looking for volume.

00:28 So i can say volume is equal to nrt.

00:31 Over p.

00:34 Okay, so now i know r &t, but i don't know v or p.

00:38 So just to deal with p first, since it's probably a little less involved.

00:42 I know the p total is equal to p of the o2, plus the pressure from water, since it's boiled over water.

00:51 Now it gives us the temperature being 40 degrees celsius, and if you check on a table, you'll find that that pressure is 55 .4 millimeters of mercury.

00:59 So essentially i have 745 millimeters of mercury is equal to this pressure plus 55 .4 millimeters of mercury.

01:15 Meaning the pressure just from the oxygen gas is going to be 689 .6 millimeters of mercury.

01:28 Okay.

01:29 So now the next thing i'm going to do is content with the moles.

01:32 The moles are going to be equal to, it says we start with 24 .78 grams of this nickel oxide...

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