Question

PART 1: Circle the best choice(s) on the test paper directly. Each multiple-choice question is worth 4 points 1. Calculate a when 33.6 g of water is heated from 22.0°C to 78.3°C. 0.991 kJ А. B C. 1.89 kJ 7.91 kJ -7.91 kJ D. 2. Determine the number of moles of this compound: 0.125 kg of the insecticide Paris Green, Cul(AsO3)2(CH3CO2)2 A. 4.94 B. 3.49 C. 0.287 D. 0.202 E. 0.2866 3. What is the net ionic equation for the reaction that occurs when aqueous solutions of NaOH and HNO3 are mixed? A. Na+ (aq) + NO3"(aq) → NaNO3(s) B. NO3"(aq) + OH"(aq) + NO3OH(s) C. H(aq) + OH(aq) → H2O(1) D. None of the above because no precipitation occurs. 4. How many moles of KOH are needed to neutralize 45.5 ml of 0.125 M H2SO4 solution? A. 5.69 x 103 moles B. 1.14 x 102 moles C. 2.84 x 10 moles D. 2.28 x 102 moles

Answer 1

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1° 33.6 g Cp of water 4.18 J/a-oc (standend valued mass of water = heat (a) mPAT 33-6 4018 (7893-220) J 7907 J 7.91 kJ 0 125 kg. 6181 Mass of insecticide Paris Green = 125 g Molar mass of Cuq (As O3)2 (CH ₂ CO2)2 = a moles of insectides Paris green almol 125 mol Маъ8 Molar mass 0.202 mol D 3. conic Net is equation for acid base reaction H+ (aq) + OH(aq) H2O(l) + 4. H₂ soy 2H+ 5042- a for each mole H₂SO4, 2 mol KOH is needed moles of H₂SO4 Molarity & volume (2) 0.125 M X 45.5 2 1000 : moles of 5.68 x 10-3 mol Koh needed - 2x moles of H2SO4 (2 x 5.68 >10-3) mol [1614x 10-2 mol B