please check if the answers for the following questions are correct :)
1) This is determined by looking at the ratio of the stoichiometric coefficients of CO to CO2, which is 3:3.2) Looking at the equation, the ratio of the number of moles of H2 that reacts to that of HCl that forms is 1:2. Thus, the number of moles of H2 that were used= 1/2(number of moles of HCl that were formed)= 1/2(12.0)= 6.0 moles3) 1.00 mole of H2O= 6.02x10^23 H2O molecules5.00 moles of H2O= 5x6.02x10^23 H2O molecules= 3.01x10^24 H2O moleculesAn H2O molecule contains 3 atoms. Thus, the number of atoms in 3.01x10^24 H2O molecules= 3x3.01x10^24= 9.03x10^24 atoms4) 1 mole of a gas occupies 22.4L at STPThus, the volume occupied by 78.0 moles of a gas at STP= (78.0x22.4)L= 1747.2L= 1747L(answer correct to 3 significant figures)5) 22.4L of a gas contains 1 mole of a gas at STPThus, the number of moles contained by 11.2L of a gas at STP= 11.2/22.4= 0.5 moles6) Since Fe is in excess, O2 is the limiting reagent, implying that all of it reacts.The ratio of the number of moles of O2 that reacts to that of Fe2O3 that forms is 3:2.Thus, the number of moles of Fe2O3 that form= 2/3(number of moles of O2 that reacts)= 2/3(6.00)= 4.00 moles7) Relative Atomic Mass(RAM) of Mg= 2424.0g= 1 mole of Mg48.6g= 48.6/24.0= 2.025 moles of MgRelative Formula Mass(RFM) of HCl= (RAM of H)+(RAM of Cl)= 1.0+35.5= 36.536.5g= 1 mole of HCl150g= 150/36.5= 4.110 moles of HClAccording to the equation, the ratio of the number of moles of Mg required to that of HCl required is 1:2. Since there is less Mg than required, Mg is the limiting reagent.8) 24.0g= 1 mole of Mg24.3g= 24.3/24.0= 1.0125 moles of Mg36.5g= 1 mole of HCl75.0g= 75.0/36.5= 2.0548 moles of HClAgain, the ratio of the number of moles of Mg required to that of HCl required is 1:2. Since there is more HCl than required, Mg is the limiting reagent, implying that all of it reacts.The ratio of the number of moles of Mg that reacts to that of MgCl2 that forms is 1:1. Therefore, the number of moles of MgCl2 that forms= the number of moles of Mg that reacts= 1.0125Relative Formula Mass(RFM) of MgCl2= (RAM of Mg)+2(RAM of Cl)= 24+2(35.5)= 951 mole of MgCl2= 95.0g1.0125 moles of MgCl2= 95.0x1.0125= 96.1875g9) False. It is actually the number of moles of each reactant that must be compared.10) Relative Atomic Mass of Hg= 200.6200.6g= 1 mole of Hg503.0g= 503.0/200.6= 2.51 moles of HgThe expected number of moles of O2 produced= 1/2(3.00)= 1.50Percent yield= (actual yield/theoretical yield)x100%= (1.25/1.50)x100%= 83.3%Relative Molecular Mass(RMM) of N2= 2(RAM of N)= 2(14)= 2828.0g= 1 mole of N284.0g= 84.0/28.0= 3 moles of N2Relative Molecular Mass(RMM) of NH3= (RAM of N)+3(RAM of H)= 14+3(1)= 1717.0g= 1 mole of NH385.0g= 85.0/17.0= 5.00 moles of NH3The expected ratio of the number of moles of N2 that reacts to that of NH3 that forms is 1:2. Thus, the percent yield= (actual amount of NH3/expected amount of NH3)x100%= (5/6)x100%= 83.3%12) Relative Molecular Mass(RMM) of SO2= (RAM of S)+2(RAM of O)= 32+2(16)= 6464.00g= 1 mole of SO264.06g= 64.06/64.00= 1.0009 moles of SO2RMM of SO3= 32+3(16)= 8080.0g= 1 mole of SO375.0g= 75/80= 0.93750 moles of SO3The expected ratio of the number of moles of SO2 that reacts to that of SO3 that forms is 1:1. Thus, percent yield= (0.93750/1.0009)x100%= 93.68%13) False. The theoretical yield can actually be calculated before the experiment has commenced by determining the the expected ratio of the number of moles of the limiting reagent to that of the product.14) True.