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Exam 4 ReviewDissociation: T / F Spectator ions appear on both sides of the reaction arrow but do not participate in the bustion analysis: Empirical formula: Actual yield: Theoretical yield: Percent yield: T / F Theoretical yield is dependent on the limiting reactantSolution: Solvent: Solute: T / F entropy is the tendency towards order T / F Increasing pressure increases solubilityIf the overall ?E is positive, the solute ________________ dissolve. If the overall ?E is negative, the solute ________________ dissolve. Predict whether a precipitation reaction will occur when the following ionic compounds are mixed together in water. If so, write the complete ionic and net ionic equation.CdCl2(aq) + (NH4)2S(aq) Ba(NO3)2(aq) + KOH(aq) How many moles are present in a 100.0g sample of glucose (C6H12O6)?How many moles of C, H, and O atoms are present in a 100.0 g sample of glucose?How many atoms are there in a 100.0g sample of glucose?Consider the unbalanced chemical equation NO + O2 NO2Balance the equation.Translate the equation into words using the word mole(s) wherever you can.To produce 2 moles of NO2 by the reaction you just wrote, how many grams of NO and O2 must you combine?What is the theoretical yield in grams of NO2?You carry out the reaction and recover 22.5g of NO2. What is the percent yield?A gaseous mixture containing 10.079 g of H2 and 7.00 moles of Br2 react to form HBr. Write the balanced chemical equation for this reaction.Which reactant is limiting?What is the theoretical yield for this reaction in moles?What is the theoretical yield for this reaction in grams?How many moles of excess reactant are left over at the end of the reaction?How many grams of excess reactant are left over at the end of the reaction?Suppose we have 2.33 moles of CH4 and 4.11 moles of O2. What is the maximum number of moles of CO2 that can be produced from this combustion reaction (hint: begin by writing a balanced chemical equation)What is the theoretical yield of Ag if 2.00g of Zn and 2.50g of AgNO3 are allowed to react?Zn(s) + 2 AgNO3(aq) Zn(NO3)2(aq) + 2 Ag(s)If after performing the reaction, the percent yield was 82%, what must have been the actual yield of Ag?What is the mass percent composition of hydrogen and nitrogen in NH3?What is the empirical formula for a compound with the following percent composition by mass? C 38.7%, H 9.76%, O 51.5% Suppose the compound was known to have a molar mass of 62.08 g/mol. Is the empirical formula the same as the molecular formula? If not, what is the molecular formula?For a solute in water, the energy changes are Esolute separation = 212 kJ, Esolvent separation = 40 kJ, and Esolvation = -480 kJ. Will this solute dissolve in water? Explain.Sodium chloride is very soluble in water but insoluble in liquid hexane, C6H14. Why is this so?When an ionic substance such as NaCl dissolves, the crystal lattice has to break apart to release the individual ions into the solution. Does this part of the dissolving process absorb energy or release energy? Explain your answer. Which one of the following steps in the dissolving process must have a negative value for ?E? Explain your answer. The physical separation of solute particlesThe formation of solvent-solute interactionsThe physical separation of solvent particlesNone of the aboveAt 100°C a saturated solution contains 5.0 g of a substance dissolved in 100 mL. Roughly how much of the substance (i.e. >5.0 g, <5.0 g, or 5 g) do you expect to be dissolved if the solution is allowed to cool to room temperature (~22°). How many grams of NaOH are needed to prepare 500.0 mL of a 0.300 M NaOH solution? How many milliliters of a 0.250 M solution of glucose, C6H12O6, are required to obtain 100.0 g of glucose?You have two solutions, one 0.755 M barium nitrate and the other 1.250 M calcium hydroxide. Write a net ionic equation for the precipitation reaction that occurs when these solutions are combined.How many milliliters of the two solutions must be combined to prepare 5.00g of precipitate?5.89 mL of a 2.84 M solution is diluted to a final volume of 18.0 L. What is the molar concentration of the final solution? ................
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