Consider the reaction: Li 2 S(aq) + Co(NO 3 ) 2 (aq) → 2 LiNO 3 (aq) + CoS(s) What volume of 0.150 M Li 2 S solution is required to completely react with 125 mL of 0.150 M Co(NO 3 ) 2 ?

Hey everyone. So here we ask calculate the volume of 0.115 moller of potassium oxide solution. That is need to react with 150 ml of 0.2 molar of Nickel Nitrate. Based on the reaction below recall that polarity. It was the most of the salute. What about leaders of the solution? And since we're given the volume in milliliters here we need to convert from male leaders. Two leaders. We have 1 50 male leaders. We have 1000 mL and one leader. And this will give us 0.15 leaders. So now we can find the moles of potassium oxide. You have 0.15 leaders. We have 0.2 molar of nickel nitrate which is going to be 0. malls of nickel nitrate in one liter. And for every one mole of nickel nitrate we're one more of potassium oxide. And this gives us 0.03 mao of potassium oxide. So now that we have malls are protesting outside and maturity of protecting oxide, we can solve for the volume. Using the maturity equation We have 0.115 smaller Equal to 0.03 laws they bought it by X. Multiply 0.115 caller times X. That equals 0.03 calls. We can solve for X. by dividing both sides by 0.115 forward. So X Equals 0.261 leaders. And since we're giving middle leaders in the question we can convert this from leaders to male leaders. We're gonna have 0.261 leaders. And in one leader we have 1000 their leaders. And this gives us 261 male leaders. Thanks for watching my video and I hope it was helpful.

Ch.4 - Chemical Quantities & Aqueous Reactions

Tro - Chemistry: A Molecular Approach 4th Edition

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Tro 4th Edition

Ch.4 - Chemical Quantities & Aqueous Reactions

Problem 66

Chapter 4, Problem 66

Consider the reaction: Li₂S(aq) + Co(NO₃)₂(aq) → 2 LiNO₃(aq) + CoS(s) What volume of 0.150 M Li₂S solution is required to completely react with 125 mL of 0.150 M Co(NO₃)₂?

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Identify the balanced chemical equation: Li_2S(aq) + Co(NO_3)_2(aq) \rightarrow 2 LiNO_3(aq) + CoS(s).

Determine the stoichiometry of the reaction: 1 mole of Li_2S reacts with 1 mole of Co(NO_3)_2.

Calculate the moles of Co(NO_3)_2 using its concentration and volume: \text{moles of Co(NO}_3\text{)}_2 = 0.150 \text{ M} \times 0.125 \text{ L}.

Use the stoichiometry of the reaction to find the moles of Li_2S needed: \text{moles of Li}_2\text{S} = \text{moles of Co(NO}_3\text{)}_2.

Calculate the volume of 0.150 M Li_2S solution required using its concentration: \text{Volume of Li}_2\text{S} = \frac{\text{moles of Li}_2\text{S}}{0.150 \text{ M}}.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows us to calculate the amounts of substances consumed and produced in a reaction based on balanced chemical equations. In this case, understanding the stoichiometric coefficients from the balanced equation is essential to determine the volume of Li2S needed to react with Co(NO3)2.

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in moles per liter (M). In this problem, both Li2S and Co(NO3)2 solutions are given in molarity, which is crucial for calculating the number of moles present in the given volumes and for determining how much Li2S is needed to react completely with the cobalt nitrate.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is key to solving stoichiometric problems, as it dictates how much of the other reactants are required. In this scenario, knowing which reactant limits the reaction will help in calculating the necessary volume of Li2S solution.