Write balanced chemical equations for the following reactions. For EACH chemical, write the coefficient in the first box, the chemical in the second box, and the state in the third box. Do not use subscripts or superscripts in your answer: for example, Caz(PO4)2 would be entered "Ca3(PO4)2". Solutions of iron (II) sulfate and calcium chloride react. iron reactant calcium reactant iron product calcium product

Write balanced chemical equations for the following reactions. For EACH chemical, write the coefficient in the first box, the chemical in the second box, and the state in the third box. Do not use subscripts or superscripts in your answer: for example, Caz(PO4)2 would be entered "Ca3(PO4)2". Solutions of iron (II) sulfate and calcium chloride react. iron reactant calcium reactant iron product calcium product

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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List the types of chemical reactions, include the generic equations (go back to the video in Module 9 about Types of Chemical Reactions if you need to refresh your memory, here is more practice, if you want to master the topic) . Classify the following chemical reactions in all possible ways (some of the chemical equations are not balanced, do NOT worry about it): C(s) + O₂(g) →→→ CO₂(g) Na(s) + Cl₂(g) →→→ NaCl(g) O H₂O(1) →H₂(g) + O2(8) CaCO3(s) CaO(s) + COz(3) CH4(8) + O₂(8) CO₂(g) + H₂O(g) O C3H8(g) + O2(8) CO2(g) + H₂O(g) O O O O C₂H5OH() + O2(8) Fe(s) + CuCl₂(aq) Cu(s) + AgNO3(aq) BaClz(aq) + Na,SO4(aq) O KBr(aq) +AgNO3(aq) O - O - CO2(8)+ H₂O(g) Cu(s) + FeCl₂(aq) Ag(s) + Cu(NO3)2(aq) →BaSO4(s)+ NaCl(aq) AgBr(s) + KNO3(aa)
10. The equations below represent precipitation reactions. Rewrite these as complete ionic and net ionic equations. Molecular Equation Complete Ionic Equation Net Ionic Equation Molecular Equation Complete lonic Equation Net Ionic Equation AgNO, (aq) + KCI (og) → KNO, (aq) + AgCl (s) Molecular Equation Complete Ionic Equation Net Ionic Equation Ba(ClO4)2 (aq) + K₂SO4 (ng) BaSO (s) + 2 KCIO₂(g) 11. The equation below represents a neutralization reaction. Rewrite this as complete ionic equations and net ionic equations. 2 HCl(aq) + Ba(OH)2 (aq) → 2 H₂O )+ BaCl₂ (aq) Include phase symbols.
Is this correct?
Write the balanced precipitation reactions
6. Sodium sulfide reacts with hydrochloric acid to produce hydrogen sulfide and sodium chloride. How many grams of sodium sulfide are required for complete reaction with 15.0 mL of 0.250 M hydrochloric acid? The molar mass of sodium sulfide is 78.046 g/mol. (Hint: start by writing the balanced equation for the reaction.)
Balance the following reaction in basic solution then enter the coefficients of the balanced reaction into the blank spaces. Remember to include "understood" coefficients of 1! 9. Type your answer here Ag20(s) + Type your answer here Al(s) + Type your answer here OH (aq) + H20(1) → Type your answer here Type your answer here Ag(s) + Type your answer here H2A!O3 (aq)
Cobalt(II) chloride solution reacts with sodium hydroxide solution. Identity the spectator ion(s). Note: you may choose more than one answer. O Co2+ Na OH
Here is some information to help. In this experiment, magnesium metal is heated until it reacts with oxygen in the air according to the following balanced equation: 2Mg(s)+ O2(g) → 2MgO(s) (silver metal) (white-gray ash) As the magnesium burns in air, it may also combine with nitrogen in air. To remove any nitride product, water is added, and the product is reheated. Any nitride product is converted to magnesium oxide and ammonia. 3Mg(s)+ N2(g) → Mg3N2(s) Mg3N2(s)+3H2O(l)→3MgO(s)+2NH3(aq) A weighed amount of the magnesium metal is used, and the mass of the oxide product formed is determined at the end of the experiment. The mass of oxygen that combines with the magnesium is obtained from the difference between the mass of the oxide product and the original mass of magnesium. mass of oxide product-mass of magnesium=mass of oxygen in oxide product The empirical formula of the oxide…
Match the following. Match the words in the left column to the appropriate blanks on the right. Make certain each blank is complete before submitting your answer. combustion oxidation-reduction precipitation acid-base gas evolution N 3. 4. 5. CH₂(g) +20₂(g) → CO₂(g) + 2H₂O(g) Reset Help H₂SO4(aq) + 2LiOH(aq) → 2H₂O(l) + Li₂SO4(aq) : Mg(s) + Cu(NO3)2(aq) → Mg(NO3)2(aq) + Cu(s) : 2HCl(aq) + (NH4)₂S(aq) → H₂S(g) + 2NH4Cl(aq) : NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq)
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Classify each chemical reaction: Ba (CIO,),(s) → BaCl,(s) + 30, (8) KOH(aq) + HBrO (aq) 1 reaction CuSO4 (aq) + Zn CrO4 (aq) K BrO (aq) + H₂O (1) CH₂OCH₂ (1) + 30₂(g) → 2CO₂(g) + 3H₂O(g) ZnSO4 (aq) + Cu Cro(s) type of reaction (check all that apply) combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition 000 000 000 precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base
For the following reaction, 72.0 grams of barium chloride are allowed to react with 64.0 grams of potassium sulfate. barium chloride(aq) + potassium sulfate(aq) →→→→→barium sulfate(s) + potassium chloride (aq) What is the maximum amount of barium sulfate that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams