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- How is stoichiometry used to calculate energy absorbed when a mass of liquid boils? A. Grams liquid x mol/g x AHyap B. Grams liquid x mol/g x A H C. Grams liquid x mol/g x AHusion O D. Grams liquid x mol/g AHeactionpls provide clear solution.les/23530384?wrap%3D1 Hwk 17 MOLE.docx OLE.docx 17 MOLE.docx (13.3 KB) ZC Hwk 17 MOLE/ MOLE STOICHIOMETRY 1) First balance the equation The combustion of a sample of butane, C,H10 (lighter fluid), produced 5.75 mol of water. C,H10 + O2 -------> CO,+ H,O a) How many moles of butane burned? b) How much oxygen was used up in moles?
- 4-During the water of crystallization Mass of an empty crucible 40.60 g. experiment, the following data were collected for the hydrated salt use them to solve Q4 and Q5 42.02 g Mass of crucible + hydrated salt Mass of crucible + anhydrous salt 41.35 Molar mass of anhydrous salt 146.5g/mol 4- The % by mass of the water in the salt equals: B. 78.1 % C. 47.2 % D. 52.8% A.21.9 %23. Solutions of sodium hypochlorite (NaClO) are sold as laundry bleach. This compound is made by the following balanced reaction. 2 NaOH + Cl2 ==> NaCl + NaClO + H2O How many g of Cl2 are needed to completely react with 9.10 g of NaOH? Give your answer to 2 decimal places. Molar Mass, g/mol NaOH 40.00 Cl2 70.91 NaCl 58.44 NaClO 74.44 H2O 18.02Use 1 decimal point for all atomic masses. 2.00 g of H2(g) are reacted with 32.0 g of O2(g) by the following reaction 2H2(g) + O2(g) --> 2H2O(g) What is the limiting reagent? H2(g) O2(g) Based on the limiting reagent, fill in the following ICE Table using moles. Enter any zero values as 0.00. H2 O2 H2O Initial Change Final How much of the excess reagent remains (in grams)?
- 12. Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below). So2(g) + H2O(1) –→ H2SO3(1) What mass of sulfur dioxide is needed to prepare 75.85 g of H2SO3(1)? Molar Mass of H2so3(1) - 82.07g/mol Molar Mass of SO2(g) - 64.07 g/mol 13. How many grams of oxygen can be obtained by the determination of 456 g of reactant in the following reaction: 2Hgo – 2Hg + 02 Molar Mass: Hg: 200.59 g/mol O: 16 g/mol| 14. How many grams of reactant are needed to obtain 97 g of oxygen in the following reaction? KCIO4 – KCI + 202 Molar Mass: K: 39.10 g/mol CI: 35.45 g/mol O: 16 g/mol 15. A reaction mixture contains 21.4 g of PC13 and 13.65 g of PBF2. What mass of PbC12 can be obtained from the reaction? Molar Mass: P: 30.97 g/mol CI: 35.45 g/mol Pb: 207.2 g/mol F: 19 g/mol 16. When 0.56 grams of CuC12 reacts with 0.64 grams of KI, how many grams of 12 is formed? Given reaction: CuC12 + KI – Cul + KCI + 12 MM CUCI2 = 110.98 g/mol MM KI = 166 g/mol MM 12 = 253.81 g/mol11. A mixture was found to contain 4.36 g of NazCO3, 6.21g of S403 and 1.89 g of LI2Se: What is the percentage of Lithium selenium?Q: A chemist attempts to prepare some crystals of borax (sodium tetraborate, Na2B,07.10H2O) by dissolving 100g of Na,B40, in 200 g of boiling water. He then carefully cools the solution slowly until some NazB407.10H2O crystallizes out. Calculate the g of NazB4O7.10H2O recovered in the crystals per 100 g of total initial solution (NazB,0, plus H2O) if the residual solution at 55°C after the crystals are removed contains 12.4% NazB4O7.
- If a bag of fertilizer were labeled as containing 35% K2O, a. What is the analysis when expressed as %K? b. Assume the bag is labeled as 150% P, calculate the percentage P2O5 in the bag.Inonngledrohedaio I inomho В. Determination of NaCl 86.096 1. Mass of evaporating dish #2, watch glass, and NaCl (g) 2. Mass of evaporating dish #2 and watch glass (g) 85.450 3. Mass of NaCI (g) calculation biuclt 4. Percent of NaCl goiuuq d biloee mod biupi calculationGiven the reaction: + HF a. Balance the reaction. 24 b. A student mixes 3.0 g N₂H with 6.33 x 10 molecules of F, gas. Determine i. The limiting reactant ii. The mass of HF gas produced if the reaction is 83.0 % efficient. NH + ____F₂- F, → ___________N₂ 2