Balance each chemical equation. b. Co(NO 3 ) 3 (aq) + (NH 4 ) 2 S(aq) → Co 2 S 3 (s) + NH 4 NO 3 (aq)

Hi everyone here, we have a question asking us to balance a fallen chemical equation cobalt nitrate plus ammonium carbonate forms, cobalt carbonate plus ammonium nitrate. So let's rewrite this. Now let's count what we have on both sides. So on our reactant side we have one cobalt we have three plus two nitrogen, so five We have three times three, so nine oxygen plus three more, so 12 oxygen. And we have four times two hydrogen, so eight hydrogen. And lastly we have one carbon. And on our product side we have to cobalt We have two nitrogen. We have three times three oxygen, so nine oxygen plus three more. So 12 oxygen. We have four hydrogen And we have three carbon. So first we're going to balance our cobalt and to do that, we're going to put a two here. So now we have two cobalt and we have two times three. So six nitrogen plus two, so eight nitrogen. And we have six Times three oxygen. So 18 oxygen. Now we're going to balance our carbon. So we're going to put a three here. So we have three times two nitrogen. So that's six plus two times three Nitrogen. So that's six. So we have 12 nitrogen And we have three Times four times 2 hydrogen. So we have 24 hydrogen And we have three carbon. We have three times three, so nine plus two times three times three. So We have 27 oxygen. And now we need to balance our nitrogen. So we're going to put a six in front of our ammonium nitrate. So we have six Plus six nitrogen, so we have 12 nitrogen. We have six times 4 hydrogen, So 24 hydrogen. We have six times three oxygen, plus three times three oxygen, So 27 oxygen. And now we are all balanced. So that is our final balanced chemical equation. Thank you for watching. Bye.

Ch.4 - Chemical Reactions and Chemical Quantities

Tro - Chemistry: A Molecular Approach 5th Edition

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Tro 5th Edition

Ch.4 - Chemical Reactions and Chemical Quantities

Problem 23

Chapter 4, Problem 23

Balance each chemical equation. b. Co(NO₃)₃(aq) + (NH₄)₂S(aq) → Co₂S₃(s) + NH₄NO₃(aq)

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Identify the number of each type of atom on both sides of the equation.

Start by balancing the metal cation, Co, by ensuring the number of Co atoms is the same on both sides.

Balance the sulfur atoms by adjusting the coefficient of (NH4)2S.

Balance the nitrogen atoms by adjusting the coefficient of NH4NO3.

Finally, balance the hydrogen and oxygen atoms, if necessary, by adjusting the coefficients of the compounds containing these elements.

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Key Concepts

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

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms for each element is the same on both sides of the equation. This is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. Coefficients are used to adjust the number of molecules or formula units to achieve balance.

Types of Chemical Reactions

Understanding the types of chemical reactions, such as double displacement, is crucial for balancing equations. In this case, the reaction between cobalt(III) nitrate and ammonium sulfide is a double displacement reaction, where the cations and anions exchange partners. Recognizing the type of reaction helps predict the products and their states.

States of Matter in Chemical Reactions

The states of matter (solid, liquid, gas, aqueous) in a chemical equation provide important information about the reactants and products. In the given equation, Co(NO3)3 and (NH4)2S are in aqueous solution, while Co2S3 is a solid precipitate. Understanding these states helps in visualizing the reaction and determining the physical changes that occur.

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Related Practice

Textbook Question

Write the balanced chemical equation for the reaction of aqueous potassium hydroxide with aqueous iron(III) chloride to form solid iron(III) hydroxide and aqueous potassium chloride.

Textbook Question

Write the balanced chemical equation for each reaction.

c. Sulfur dioxide gas reacts with oxygen gas to form sulfur trioxide gas.

d. Gaseous ammonia (NH₃) reacts with gaseous oxygen to form gaseous nitrogen monoxide and gaseous water.

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Textbook Question

Consider the unbalanced equation for the neutralization of acetic acid: HC₂H₃O₂(aq) + Ba(OH)₂(aq) → H₂O(l) + Ba(C₂H₃O₂)₂(aq) Balance the equation and determine how many moles of Ba(OH)₂ are required to completely neutralize 0.461 mole of HC₂H₃O₂.

Textbook Question

Calculate how many moles of NO₂ form when each quantity of reactant completely reacts. 2 N₂O₅( g) → 4 NO₂(g) + O₂(g) a. 2.5 mol N₂O₅

Textbook Question

Calculate how many moles of NH₃ form when each quantity of reactant completely reacts. 3 N₂H₄(l) → 4 NH₃(g) + N₂(g) c. 65.3 g N₂H₄

Balance each chemical equation. b. Co(NO3)3(aq) + (NH4)2S(aq) → Co2S3(s) + NH4NO3(aq)

Verified video answer for a similar problem:

Key Concepts

Balancing Chemical Equations

Types of Chemical Reactions

States of Matter in Chemical Reactions

Balance each chemical equation. b. Co(NO₃)₃(aq) + (NH₄)₂S(aq) → Co₂S₃(s) + NH₄NO₃(aq)