Chemical Reactions AssignmentPredict whether or not each of the following reactions will occur. Write thebalanced chemical equation for each of the reactions that can occur. If areaction would not occur, write: 'no reaction'.1. Potassium plus copper (II) chloride |2. Zinc plus lead (II) nitrate3. chlorine plus potassium iodide4. barium oxide plus liquid water5. silver plus hydrochloric acid6. aluminum plus oxygen7. bromine plus potassium iodide8. magnesium plus steam (gaseous water)9. gold plus hydrochloric acid10. magnesium plus cobalt (II) nitrateComplete the reactions and balance the reactions1. 2LiCl(aq) + Pb(NO3)2(aq) →2. H₂SO3(aq) →3. Ba Cl₂ (aq) + Na₂ CrO4(aq) →4. H₂SO4(aq) + Ca(OH)₂(aq) →5. Potassium Sulfate (aq) + Calcium chloride (aq) →Note: write the chemical reaction by chemical formulas the sameas numbers 1-4

Note:Since you have posted multiple questions with multiple sub parts, we will provide the solution…

Chemical Reactions Assignment Predict whether or not each of the following reactions will occur. Write the balanced chemical equation for each of the reactions that can occur. If a reaction would not occur, write: 'no reaction'. 1. Potassium plus copper (II) chloride 2. Zinc plus lead (II) nitrate 3. chlorine plus potassium iodide

Chemical Reactions Assignment Predict whether or not each of the following reactions will occur. Write the balanced chemical equation for each of the reactions that can occur. If a reaction would not occur, write: 'no reaction'. 1. Potassium plus copper (II) chloride 2. Zinc plus lead (II) nitrate 3. chlorine plus potassium iodide

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...

See similar textbooks

Similar questions

Consider a double replacement reaction between Zinc (ll) chloride and sodium hydroxide: ZnCl2+NaOH ==> Complete the chemical equation by: 1. Rewriting it to include electrically-neutral ionic product formulas for each formula. To clarify instead of just writing the product formulas rewrite the entire equation. Concerning the "electrically neutral" part, you are reminded that if for example, Na + Cl2 ==> were your reactants, you would not predict NaCl2 as a chemical product because that is not an electrically neutral compound formula. The Na would have a +1 charge and, the Cl would have a -1 charge, 2 (-1) charges would give an overall -2 charge which would not produce an overall 0 charge. 2. Balance it. 3. Add subscripts (aq, I, s, or g) to show how the reactants combine and which product will precipitate to be collected as a solid. 4. Provide subscripts for both reactants and both products.
A. Classify the given chemical equations and scenarios as to SYNTHESIS, DECOMPOSITION, SINGLE REPLACEMENT, DOUBLE REPLACEMENT, or COMBUSTION reaction.
1. What is the general equation that represents a single displacement reaction?
For each question, do the following four things: 1. Predict the products that will be made in this double replacement reaction. 2. Write the formulas for each substance. 3. Record the states of matter. 4. Balance the equation.
1. Write the correct chemical equation for the following reaction: when beryllium chloride reacts with silver (I) nitrate, beryllium nitrate and silver (I) chloride are formed 2. Write the correct skeleton equation for the following: fluorine gas reacts with calcium metal to form solid calcium fluoride
Directions: Write and balance the chemical equation of the following wordequations.9. The decomposition of solid barium nitrate leads to the formation of solid barium oxide,diatomic nitrogen gas, and diatomic oxygen gas.10. Write an equation for the reaction of solid silicon dioxide with hydrofluoric acid to yieldgaseous silicon tetrafluoride and liquid water.
How can we represent a chemical reaction with a chemical equation? Provide an example?
Balancing Chemical Equations Determine the type of reaction occurring placing P (precipitation), N (acid-base neutralization), R (redox) on the line in front of the reactants. Predict the names of the products, placing them on the lines provided, AND whether a reaction will occur. Write balanced equations as indicated for each reaction, showing state symbols for reactions that will occur. Write NNR for the reactions that will not occur: 1. sodium iodide + lead (II) nitrate → Molecular Reaction: Total Ionic Reaction: Net Ionic Reaction:
A solution of zinc acetate and a piece of aluminum metal are mixed together in a test tube. For the following reaction, a) Determine the type of reaction, and bi) if the reaction occurs, write the balanced reaction, including all states of matter, or bii) if the reaction does not occur, explain why the reaction does not occur.
For each of the following sets of reactants, write the balanced equation for the single displacement reaction that occurs. If you determine that a reaction will not occur, write “NR”, and provide a brief explanation. a. Aluminum metal + aqueous nickel(II) nitrate b. Gold metal + hydrobromic acid
Question 6 of 21 Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 4.78 g of magnesium ribbon burns with 7.61 g of oxygen, a bright, white light and a white, powdery product are formed. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. equation: What is the limiting reactant? O oxygen magnesium The reaction goes to completion, but in the process of recovering the product, some of it was lost. The the percent yield for the reaction is 82.8%. How many grams of product are recovered? mass of product recovered: g How many grams of the excess reactant remain? Assume the reaction goes to completion. mass of excess reactant:
(write a balanced chemical equation with accurate states) Phosphoric acid solution removes iron(III) hydroxide stains from an old bath tub.