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- 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?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 18.029. How many moles of 2 Na(s) * 24- 2. Provide an example calculation for row 8. This requires you to go from g CO2 to g NaHCO3 using stoichiometry. Use equation 2, a net ionic equation for the reaction of acid, H3O* (from acetic acid, CH3COOOH in vinegar) with the bicarbonate (from NaHCO3 in pill) to determine the molar ratio for your calculation. Note that Na+ (aq) doesn't show up in this equation because it is a spectator ion. Hag) H
- Use 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)?P4(s) + _Cl2(g) → _PCI5(g) AH°rxn = -1500 kJ balance & classify: - -- The reaction is _thermic, heat flows bonds between atoms become er In a reaction mixture of 0.22 g(P4) and 1.45 g(Cl2): significant figures! The 0.22 grams of P4 are enough to form mol(PCI5) LSTP (PCI5) The 1.45 grams of Cl, are enough to form mol(PCI5) LSTP (PCI5) The limiting reagent (LR) in the mixture is The theoretical yield of PCI5 is mol and LSTP (liters at STP) If 0.12 LSTP(PCI5) was isolated, the percent reaction yield is % The most heat this reaction mixture can form is kJ5) If all the NaHCO3 in bag 2 reacted, calculate the number of moles of gas produced? tates) E Focus
- 9Mass of Na2CO3.H2O (g) = 2.12g (g) Mass of the CaCl2.2H2O (g) = 1.98g Mass of the top funnel + filter paper (g) = 15.85g Mass of top funnel + filter paper + CaCO3 collected (g) = 17.81g CaCl2 + Na2CO3 ==== CaCo3 + 2NaCl Moles CaCO3 produced by Na2CO3 (if all Na2CO3 reacts)? Moles CaCO3 produced by Na2CO3 (if all CaCl2 reacts)? What is the Limiting Reagent? Moles Na2CO3 reacting? Moles CaCl2 reacting?Use 1 decimal point for all atomic masses. 12.1 g of C2H4(g) are reacted with 0.924 g of HCl(g) by the following reaction: C2H4(g) + HCl(g) --> C2H5Cl(g) What is the limiting reagent? HCl(g) C2H4(g) Based on the limiting reagent, what should the yield of C2H5Cl(g) be?
- cetic Acid Aspirin 1on se 0 ag nol) 1stbo nn sved nenonbyil nedt 1adio 2mole e in Consider the reaction below and find the limiting reagent and theoretical yield when 5.0 g of 1-hexene is reacted with 10.0 g of hydrobromic acid. Br H2 .C. H2 .C. CH3 CH CH3 +HBr %3D H2C C. H2 H3C H2 H2 H2 2-bromohexane 1-hexeneUse 1 decimal point for all atomic masses. 82.1 g of Ni3C(s) are reacted with 1.80 g of H2(g) by the following reaction: Ni3C(s) + 2H2(g) --> 3Ni(s) + CH4(g) What is the limiting reagent? H2(g) Ni3C(s) Based on the limiting reagent, what should the yield of Ni be?Samples of hydrated manganese perchlorate are heated to determine the amount of crystal water: Mn(CIO4)2 nH20 -» Mn(CIO4)2 nH20 A sample of 2.126 g weighs 1.473g after heating. The mass of water that evaporated is: The molar ratio of water to manganese perchlorate up to two decimal points is: a.u