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An unknown hydrocarbon was burned to produce 44 grams of CO2 and 18 grams of H2O, What is the empirical formula of this hydrocarbon? a) CH b) CH2 c) C2H d) CH4

In a PES diagram of Magnesium, which peak would show the most energy? a) 3s b) 2p c) 1s a) 2s

Which of the following ions has the smallest ionic radius? a) Na+ b) Mg+2 c) F- d) Cl-

If a sample of a solution of copper sulfate is doubled in concentration, the absorption of light in that sample would a) stay the same b) quadruple c) decrease by ½ d) double

What type of radiation would cause molecules to have vibrational motion? a) Ultraviolet c) Microwave b) Infrared d) X-rays

Using paper chromatography, if a mixture of molecular compounds is dissolved in hexane(C6H12), which component in the mixture will go the highest up the paper a) The most nonpolar substance b) The most polar substance c) The most dense substance d) The least dense substance

Iron is made stronger by alloying it with carbon Iron is made stronger by alloying it with carbon. The factor that gives this alloy it’s improved properties is due to the fact that compared to iron, carbon a) is a nonmetal b) has a smaller atomic radius c) has a lower melting point d) has a lower density

a) NaCl b) LiCl c) CaO d) MgO Based on Lattice energy and Coulomb’s Law, which ionic compound has the greatest melting point? a) NaCl b) LiCl c) CaO d) MgO

One mole of an ideal gas has a volume of 22. 4 L at STP One mole of an ideal gas has a volume of 22.4 L at STP. However one mole of SO2 has a volume less than 22.4L at STP. What is the best explanation for this? a) SO2 particles are larger than those of an ideal gas b) Both Sulfur and Oxygen are in the same group of the periodic table c) SO2 has intermolecular forces that cause the molecules to take up less space d) SO2 has a larger molar mass than most ideal gases

An unknown substance shows properties of malleability An unknown substance shows properties of malleability. Which attribute explains this property? a) low density b) high ionization energy c) high electronegativity d) delocalzed electrons

A + 2B C In the above reaction, how many moles of C will be formed when 2 moles of A reacts with 2 moles of B (assume the reaction goes to completion). a) ½ a mole b) 2 moles c) 1 mole d) 3 moles

AgNO3 reacts with NaCl in an exothermic reaction AgNO3 reacts with NaCl in an exothermic reaction. What evidence would be used to prove that this chemical reaction has occured? a) a gas was released b) the reaction dropped in temperature c) a precipitate was formed d) there was a change in pressure

Mg + Al+3 Mg+2 + Al In the above reaction, how many moles of electrons are transferred, once it is balanced? a) 3 b) 6 c) 2 d) 1

A battery is made using the two ½ reactions listed below A battery is made using the two ½ reactions listed below. Calculate the cell potential of this reaction given the reduction potentials listed below. Ag+ + e- Ag Eored = 0.80 Volts Zn+2 + 2e- Zn Eored = - 0.76 Volts a) 0.04 volts b) -0.04 volts c) 1.56 volts d) 3.16 volts

Zn + Cu+2 Zn+2 + Cu In the above reaction, the Eocell is 1.10 volts. What would happen to the voltage of the cell if the concentration of the Cu+2 ions were increased to 2M while the concentration of the Zn+2 remained tat 1M? a) voltage would be less than 1.10 volts b) voltage would be 0 c) voltage would be greater than 1.10 volts d) there would be no change in the volts

In the reaction A + B C, when the concentrations of both A and B were doubled, the reaction rate also doubled. Which of the following could explain this result? a) The reaction was 1st order in A and B b) The reaction was 2nd order in A and B c) The reaction was 1st order in A and zero order in B d) The reaction was 2nd order in A and 1st order in B

What method could a student use to determine that a reactant is first order? a) The reaction is a two step mechanism b) the concentration of the reactant decreased over time c) when the temperature was increased, the rate of the reaction increased d) the ½ life of the reactant was independent of its concentration

A hot metal object is dropped into 100 g of water at 30oC A hot metal object is dropped into 100 g of water at 30oC. The heat absorbed by the water was 4.2 kJ. What was the final temperature of the water? (Specific Heat Capacity of water is 4.2J/goC) a) 20 oC b) 40 oC c) 31 oC d) 29 oC

A sample of I2 sublimates slightly above room temperature A sample of I2 sublimates slightly above room temperature. The best reason for this is due to? a) weak non-polar bonds b) weak London Dispersion Forces c) Iodine’s high electronegativity d) Iodine’s high ionization energy

An endothermic reaction observed to occur with the formation of a gas from solid reactants. The reaction was thermodynamically favorable a) at high pressures b) at any temperature c) only at low temperatures d) only at high temperatures

For the reaction A(g) + B(g)   2C(g) Kp = 200 at 25oC. A mixture of the three gases is placed in a reaction flask and the initial pressures were PA = 10 atm, PB = 10 atm, and PC = 5 atm. At the instant of mixing a) the rxn will produce more A because K>1 b) the rxn will produce more A because Q<K c) the rxn will produce more C because Q>K d) the rxn will produce more C because Q<K

If 100 mL of 0. 1M acetic acid was titrated with 40 mL of 0 If 100 mL of 0.1M acetic acid was titrated with 40 mL of 0.1M NaOH what would be the approximate pH given that the pKa of acetic acid is 4.74? a) pH >4.74 b) pH <4.74 c) pH = 4.74 d) can not be determined

Which of the following 0.1M solutions would produce a buffer with a pH around 9? Buffer solution a) NH3/NH4Cl Kb of NH3 = 1.8x10-5 b) HC2H3O2/NaC2H3O2 Ka of HC2H3O2 = 1.8x10-5 c) HF/NaF Ka of HF = 3.5 x10-4 d) C6H5NH2/(C6H5)NH3Cl Kb of (C6H5)NH2 = 3.8x10-10

A 0. 1M solution of MgCl2 is added to a buffer with a pH of 10 A 0.1M solution of MgCl2 is added to a buffer with a pH of 10. Which of the following statements is correct? (The Ksp of Mg(OH)2 is 1.8 x10-11) a) Mg(OH)2 will precipitate because Q<K b) Mg(OH)2 will precipitate because Q>K c) Mg(OH)2 will not precipitate because Q>K d) Mg(OH)2 will not precipitate because Q<K

Two 100 mL portions of 0.1M acids, HX and HY, are added to two100 mL portions 0.1M NaOH solutions. It was determined that HX was the weaker acid because a) HX had a pH >1 at the start of titration b) ½ way to the equivalence point HX’s pH= pKa c) HY had aa higher pH than HX at the equivalence point d) HX had a higher pH than HY at the equivalence point

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