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(a)
Interpretation:
To determine the balanced equation for the given reaction - When solid ammonium nitrite is heated, it produces nitrogen gas and water vapour.
Concept Introduction:
The balanced chemical equation is the equation in which number of different atoms of elements in the reactant side is equal to products side.
(b)
Interpretation:
To determine the balanced equation for the given reaction - Gaseous nitrogen monoxide (common name, nitric oxide) decomposes to produce dinitrogen monoxide gas (common name, nitrous oxide) and nitrogen dioxide gas.
Concept Introduction:
It is required that one can determine the reactants and products of the given statement and their respective states and write the unbalanced equation first. Then, balance it and determine the balanced equation. The balanced chemical equation is the equation in which number of different atoms of elements in the reactant side is equal to products side.
(c)
Interpretation:
To determine the balanced equation for the given reaction - Liquid nitric acid decomposes to reddish-brown nitrogen dioxide gas, liquid water, and oxygen gas (This is why bottles of nitric acid become yellow upon standing).
Concept Introduction:
It is required that one can determine the reactants and products of the given statement and their respective states and write the unbalanced equation first. Then, balance it and determine the balanced equation. The balanced chemical equation is the equation in which number of different atoms of elements in the reactant side is equal to products side.
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Chapter 6 Solutions
Introductory Chemistry: A Foundation
- Practice Exercise 1The unbalanced equation for the reaction between methaneand bromine is__ CH41g2 + __ Br21l2¡__ CBr41s2 + __ HBr1g2Once this equation is balanced, what is the value of thecoefficient in front of bromine Br2?(a) 1 (b) 2 (c) 3 (d) 4 (e) 6arrow_forwardExercise: Assume that 10g of K-PtCl, and 10g of NHare allowed to react, how many grams of the excess reactant are consumed, and how many grams remain? R KPtCla + 2NH3 Pt(NH)Cl+ 2KCIarrow_forwardExercise: Write the word equation of the following: 1. The complete combustion of gasoline yields carbon dioxide, water vapor and a great amount of heat. 2. In an electrolytic cell, water decomposes into its elements hydrogen gas and oxygen gas. 3. Sulfuric acid neutralizes sodium hydroxide to give sodium sulfate and water. 4. Ferrous nitrate reacts with potassium hydroxide to give a green precipitate of ferrous hydroxide and potassium nitrate. 5. Methane is known as marsh gas. It is a good fuel. Methane burns with the oxygen of the air to produce carbon dioxide and water vapor. 6. The complete combustion of the hydrocarbon pentane.arrow_forward
- Evaluation 2 Write the chemical equivalent of the following chemical reactions with their substance states. 1. Zinc metal reacts with a solution of sulfuric acid to produce a solution of zinc sulfate and hydrogen gas. 2. Copper (II) oxide reacts with aluminum to give aluminum oxide and copper.arrow_forwardFor the following reaction, 0.553 moles of potassium hydroxide are mixed with 0.555 moles of phosphoric acid. potassium hydroxide (aq) + phosphoric acid (aq) → potassium phosphate (aq) + water(!) What is the formula for the limiting reagent? Limiting reagent: What is the maximum amount of potassium phosphate that can be produced? Amount moles Submit Answer Try Another Version 10 item attempts remainingarrow_forwardExplain and elaborate. Don't copy paste.arrow_forward
- Can Do It Exercise 1: In the below setup, iron is added to acid in a flask fitted with empty balloon. The mass o the setup is noted using digital balance. 525.6 K 325.6 g 525.6 M Before Reaction During Reaction At End of Reaction chemix.org 1- What is the evidence for this reaction? 2- Based on the figure, fill the table with the correct data Before Reaction At end of reaction Substances in flask & balloon Balloon (empty/ filled) Mass of setup 3- Compare the masses before and at end of reaction. 4- What do you conclude? 5- Write the word equation of the reaction.arrow_forwardAcetylene is the substance burned in oxy-acetylene torches. Write a balanced equation for the complete oxidation reaction that occurs when acetylene (C,H,) burns in air. Use the smallest possible integer coefficients. Submit Answer Try Another Version 10 item attempts remaining Previous Nextarrow_forwardPlease correct answer and don't use hand ratingarrow_forward
- Exercise 5.69 53 of 54 MISSED THIS? Read Section 5.9 I Review I Constants I Periodic Table (Pages 193 - 201). Which metal could you use to accomplish this? Suppose you wanted to cause Ni?+ ions to come out of solution as solid Ni. Activity Series of Metals Mg(s) → Mg²+*(aq) + 2e Al(s) → Al³+ (aq) + 3e Mn(s) → Mn²+(aq) + 2e¯ Strongest tendency to lose electrons Most reactive Most easily oxididized → Zn²+(aq) + 2e Cr+ (aq) + 3e + Fe²+(aq) +3e Zn(s) Cr(s) Fe(s) Ni²+ (aq) + 2e¯ → Sn²*(aq) + 2e Pb(s) → Pb²+(aq) + 2e¯ Ni(s) Sn(s) H2 (g → 2H (aq)+ 2e Cu(s) Ag(s) Au(s) → Au+ (aq) + 3e Cu²+(aq) + 2e → Ag* (aq)+e Least reactive Most difficult to oxidize Least tendency to lose electrons Check all that apply. O Zn O Mg O Cu O Pb O Fe Submit Request Answerarrow_forward#3arrow_forwardPRACTICE EXERCISE : Problem Solving N2 + 3H2 --> 2NH3 How many grams of H2 are needed to react with 4.5 moles of N2? Step 1. Identify the problem. Step 2. Identify the conversion factor based from the balanced chemical equation. Step 3. Find out the number of moles using the Dimensional Analysis. Step 4. Change the moles using the molar mass.arrow_forward
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
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