Categorize the following reactions as synthesis, decomposition, or exchange reactions in the forward direction Drag the appropriate items to their respective bins. Decomposition FeCl(aq) + 2NaOH(aq)+ Fe(OH),()+2NaCl(aq) Exchange 4HC1(g) + O₂(g) 28,0(x) +20%,() CO₂(e)+C) 200(g) Synthesis 3

Categorize the following reactions as synthesis, decomposition, or exchange reactions in the forward direction Drag the appropriate items to their respective bins. Decomposition FeCl(aq) + 2NaOH(aq)+ Fe(OH),()+2NaCl(aq) Exchange 4HC1(g) + O₂(g) 28,0(x) +20%,() CO₂(e)+C) 200(g) Synthesis 3

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Consider each chemical equation and select all that represent a chemical reaction. 2NaI(aq) + Pb(NO3)2(aq) → 2NaNO3(aq) + PbI2(s) 2KBr(aq) + MgCl2(aq) → 2KCl(aq) + MgBr2(aq) HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s)+CuSO4(aq)→Cu(s)+FeSO4(aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 350.mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 142.mg. Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.
The reaction for producing glucose in plants, called photosynthesis, is 6CO2+6H2O−→−−lightC6H12O6+6O2 6CO2+6H2O→lightC6H12O6+6O2 If a plant produces 7.56 mol C6H12O6,7.56 mol C6H12O6, how many moles of CO2CO2 are needed?
One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe (s) + CuSO4 (aq) → Cu (s) + FeSO4 (aq)Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 200.mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 73.mg . Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.
One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO4(aq) → Cu(s) + FeSO4 (aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 350. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 111. mg. Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits. 0-2 X 5
The reaction A(aq) + B(aq) C(aq) + D(aq) has a ΔHrxn = -85 kJ/mol. This reaction is endorthermic or exothermic . If the temperature of the reaction mixture is increased, equilibrium will shift towards the reactans or products. This change will decrease or increase the concentration of the reactants and K will increase or deacrease
Which of the following statements is a true statement concerning a reaction that has reached a state of equilibrium? A system has reached equilibrium when the concentrations of reactants and products remain constant. A system has reached equilibrium when the reaction has stopped and no more products are formed. A system has reached equilibrium when the rate constant for the forward reaction equals the rate constant of the reverse reaction. A system has reached equilibrium when the concentrations of reactants and products correspond to the stoichiometric ratios determined by the balanced equation.
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