Instructions for Chemistry take - home test:1. Solve the exercises below.2. Include all the calculations made and the units, when solving the exercise.3. Remember to include the states of reactants and products in chemical reactions.1) Calculate the molecular masses of NaC2H3O, Fe2(SO4)3, NHẠNO3, NaCl, H2O, and CH3COOH.Use these values if you need them elsewhere in the exam.Atomic weight22.99 g/mol32.07 g/mol1.01 g/mol12.01 g/mol55.85 g/mol16.00 g/mol35.45 g/mol14.01 g/molElementNaSHCFeClN2) Heating 2.50g of NaC2H3O × H2O gave 1.50g of the residue.Calculate:mass of water lostb. percentage of water in the hydratec. moles of waterd. moles of anhydrous salte. molar ratio of water (X)The correct chemical formula of the hydrate is:I.a.II.3) Complete, balance, and classify the following reactions. Identify the reaction in decomposition,combination, combustion, single displacement, and double displacement. In the case of doubledisplacement, indicate whether it is neutralization, precipitation, or gas formation.NİSO4 +7 H2O (s) →Reaction type:а.b.Na3PO4(ac) →FeSO4(ac) +Reaction type:H2(g) +Reaction type:с.O2(R)K2CO3(ac) +Reaction type:d.HCl(ac) →Alo +Reaction type:HNO3(ac) +Reaction type:е.HCl(ac) →f.Вa (ОН)2ас) —>

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3. Remember to include the states of reactants and products in chemical reactions. 1) Calculate the molecular masses of NaC;H3O, Fe2(SO4)3, NHẠNO3, NaCl, H2O, and CH3COOH. Use these values if you need them elsewhere in the exam. Atomic weight 22.99 g/mol 32.07 g/mol 1.01 g/mol 12.01 g/mol 55.85 g/mol 16.00 g/mol 35.45 g/mol 14.01 g/mol Element Na H Fe Cl

3. Remember to include the states of reactants and products in chemical reactions. 1) Calculate the molecular masses of NaC;H3O, Fe2(SO4)3, NHẠNO3, NaCl, H2O, and CH3COOH. Use these values if you need them elsewhere in the exam. Atomic weight 22.99 g/mol 32.07 g/mol 1.01 g/mol 12.01 g/mol 55.85 g/mol 16.00 g/mol 35.45 g/mol 14.01 g/mol Element Na H Fe Cl

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 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.
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4. You dissolve 50 grams of CaBr2 and 100 grams of Ca(NO3)2 into the same 2.50 liters of water. No chemical reaction happens. Calculate the moles of CaBr2 Calculate the moles of Ca(NO3)2 •No volume conversion is needed. Volume is already in liters. • Write the balanced dissociation equations for CaBr₂ and Ca(NO3)2 Calculate the molarity of CaBr2₂ in the solution. • Calculate the molarity of Ca(NO3)2 in solution. • Calculate the molarity of the Ca²+, NO3, and Br in the solution. Formula Mass of CaBr₂ = Formula Mass of Ca(NO3)2 = Moles CaBr₂ = Moles Ca(NO3)2 = Volume (1) = Dissociation Equation CaBr2 Dissociation Equation Ca(NO3)2 [CaBr₂] = [Ca(NO3)2] = [Ca²+] = [Br] =[ NO; ] = Answer Your calculations & equations
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Use the conservation of mass interactive to answer the questions. Consider the reaction. MnS(s) + 2 HCI(aq) __ MnCI2(aq) +H2S(g) if the large amount of MnS is combined with large amount HCI, what is the mass of the products? The mass of any excess reaction will also be included in this total
CHAPTER 8 - SOLUTIONS Previous Page 18 of 35 Next O If 8.50 g Ca(NO3)2 is dissolved in enough water to make 0.750 L of solution, what is the molar concentration of Ca(NO3)2?
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An acid, HEl, is formed from a hypothetical element, El, and a subsequent aqueous solution is created with the acid and water. The solution is measured to be 20.09% HEl by weight. Calculate the mol % of the acid in the solution. Atomic Mass: H: 1.00784 g/mol O: 15.999 g/mol El: 142.93023 g/mol
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