Transcription of Practice Test Ch 3 Stoichiometry Name Per
1 Remember, this is Practice - Do NOT cheat yourself of finding out what you are capable of doing. Be sure you follow the testing conditions outlined below. DO NOT USE A CALCULATOR. AP Chem does not allow the use of a calculator for the MC part of the exam, so it is time to start practicing without one. You may use ONLY a periodic table. While you should Practice working as fast as possible, it is more important at this point in the course, that you Practice without a calculator, even if it slows you down.
2 Look for the easy math common factors and rough estimation do not do long division to try to get exact values. Remember it is a MC test, use the answers Mark which questions you would like to go over when we get to school in the following equation:___NH3 + ___O2 ___NO2 + ___H2 OThe balanced equation shows that mole of NH3 requires ___ mole(s) of a balanced equation for the combustion of acetaldehyde, properly balanced, the equation indicates that ___ mole(s) of O2 are required for each mole of is the total mass of products formed when 16 grams of CH4 is burned with excess oxygen?
3 G g g a balanced equation for the combustion of propane, balanced, the equation indicates that ___ moles of O2 are required for each mole of the following equation with the SMALLEST WHOLE NUMBER COEFFICIENTS possible. Select the number that is the sum of the coefficients in the balanced equation:___KClO3 ___KCl + the mass of hydrogen formed when 27 g of aluminum reacts with excess hydrochloric acid according to the balanced equation + 6 HCl 2 AlCl3 + 3 g many grams of nitric acid, HNO3, can be prepared from the reaction of 138 g of NO2 with g H2O according to the equation below?
4 3NO2 + H2O 2 HNO3 + of the following statements is true? molar mass of CaCO3 is g mol g of CaCO3 contains 9 1023 oxygen 200 g sample of CaCO3 contains 2 moles of and III , II, and III Practice Test Ch 3 Stoichiometry Name_____Per_____2 MnO2 + 4 KOH + O2 + Cl2 2 KMnO4 + 2 KCl + 2 the reaction above, there is 100. g of each reactant available. Which reagent is the limiting reagent?[Molar Masses: MnO2 = ; KOH= ; O2 = ; Cl2 = ] all run out at the same reaction of g benzene, C6H6, with excess HNO3 resulted in g of H2O.
5 What is the percentage yield?Molar Mass (g/mol): C6H6=78 HNO3=63 C6H5NO2=123 H2O=18C6H6 + HNO3 C6H5NO2 + many grams of H2O will be formed when g H2 is allowed to react with g O2 according to2 H2 + O2 2 g g of H2 reacts with g of O2 in an explosion, the final gas mixture will , H2O, and and H2O and H2O only and O2 g of metal carbonate, containing an unknown metal, M, were heated to give the metal oxide and g (s) + heat MO(s) + CO2(g)What is the identity of the metal M?
6 Given sample of some hydrocarbon is burned completely and it produces g of CO2 and g of H2O. Determine the empirical formula of the simplest formula for a hydrocarbon that is percent hydrogen by mass mass of Al is produced when mole of Al2S3 is completely reduced with excess H2? g a sample of an unknown mineral was dissolved in acid, of CO2 were generated. If the rock contained no carbonate other than MgCO3, what was the percent of MgCO3 by mass in the limestone?Molar mass (g/mol): MgCO3 = 84 and CO2 = of the following represents the correct method for converting g of copper metal to the equivalent number of copper atoms?
7 10231 1023 10231 1023 Practice Test Ch3 Stoichiometry (page 2 of 2) mass of element X found in mole of each of four different compounds is g, g, g, and 70 g, respectively. The possible atomic weight of X (g) + 2O2(g) N2O4(g) above reaction takes place in a closed flask. The initial amount of N2(g) is 8 mole, and that of O2(g) is 12 mole. There is no N2O4(g) initially present. The experiment is carried out at constant temperature.
8 What is the total amount of mole of all substances in the container when the amount of N2O4(g) reaches 6 mole? mole that there are two naturally occurring isotopes of gallium, 69Ga and 71Ga, the natural abundance of the 71Ga isotope must be % % % % %2Ca3(PO4)2 + 10C + 6 SiO2 P4 + 6 CaSiO3 + phosphorus can be produced by the reduction of phosphate minerals in an electric furnace. What mass of carbon would be required to produce mol of P4 in the presence of 1 mol of calcium phosphate and 3 mol of silicon dioxide?
9 G which of the following compounds is the mass ratio of element X to oxygen closest to to 1? (The molar mass of X is g/mol.) 6H+ + 5H2O2 + 2 MnO4 5O2 + 2Mn2+ + to the balanced equation above, how many moles of the permanganate ion are required to react completely with ml of M hydrogen peroxide? mol molFor the Free Response you may use a calculator and Periodic g sample containing calcium carbonate and an inert material was placed in excess hydrochloric acid.
10 A reaction occurred producing calcium chloride, water, and carbon dioxide.(a)Write a balanced equation for the reaction.(b)When the reaction was complete, g of carbon dioxide gas was collected. How many moles of calcium carbonate were consumed in the reaction?(c)If all the calcium carbonate initially present in the sample was consumed in the reaction, what percent by mass of the sample was due to calcium carbonate?(d)If the inert material was only silicon dioxide, what was the mole fraction of silicon dioxide in the mixture?
