last chemistry test .. Really need this test to be aced !
Question 1 (Multiple Choice Worth 2 points)[07.06]In the chemical reaction shown below, which element was reduced?Zn + H2SO4 ZnSO3+ H2O[removed] Zn, because it gained 2 electrons[removed] Zn, because it lost 2 electrons[removed] S, because it gained 2 electrons[removed] S, because it lost 2 electronsQuestion 2 (Multiple Choice Worth 2 points)[05.03]If 1.6 moles of an ideal gas are at a temperature of 25°C and a pressure of 0.91 atm Hg, what volume would the gas occupy, in liters?[removed] 0.28 L[removed] 3.0 L[removed] 36 L[removed] 43 LQuestion 3 (Multiple Choice Worth 2 points)[05.01]Which phase of matter is made up of particles that are packed relatively close together, with an indefinite shape but a definite volume?[removed] gas[removed] liquid[removed] plasma[removed] solidQuestion 4 (Multiple Choice Worth 2 points)[06.04]Which of the following circumstances will result in a reaction that is spontaneous only at low temperatures?[removed] positive enthalpy change and positive entropy change[removed] negative enthalpy change and negative entropy change[removed] positive enthalpy change and negative entropy change[removed] negative enthalpy change and positive entropy changeQuestion 5 (Multiple Choice Worth 2 points)[08.03]Which of the following best describes the forces that create natural gas?[removed] Heat from the Earths core and pressure transform the remains of dead plants and animals.[removed] Energy of the sun strikes photovoltaic cells producing a flow of electrons.[removed] Heat energy beneath the Earth’s surface heats underground water into steam.[removed] Heat energy is released during nuclear fission and steam is produced to turn a turbine.Question 6 (Multiple Choice Worth 2 points)[07.06]Which of the following chemical reactions is an oxidation-reduction reaction?[removed] Fe2O3 + 3CO 2Fe + 3CO2[removed] MgSO4 + 2KI K2SO4 + MgI2[removed] NaNO3 + KCl KNO3 + NaCl[removed] Cu(NO3)2 + 2HBr CuBr2 + 2HNO3Question 7 (Multiple Choice Worth 2 points)[08.01]Which of the following represents a balanced nuclear equation showing Bismuth-212 undergoing alpha decay followed by beta decay?[removed] + x- +[removed] + + x-[removed] + +[removed] + +Question 8 (Multiple Choice Worth 2 points)[07.03] What is the concentration of hydronium ions in a solution with a pH = 3.9?[removed] 4.14 × 10-2[removed] 7.80 × 10-3[removed] 1.26 × 10-4[removed] 3.00 × 10-5Question 9 (Multiple Choice Worth 2 points)[07.02]Which of the following is the salt in the Brønsted-Lowry neutralization reaction?HBr + NaHCO3 H2CO3 + NaBr[removed] HBr[removed] NaHCO3[removed] H2CO3[removed] NaBrQuestion 10 (Multiple Choice Worth 2 points)[05.07]How many grams of potassium nitrate (KNO3) would form if 2.25 liters of a 1.50 molar lead nitrate Pb(NO3)2 solution reacts with 1.15 liters of a 2.75 molar potassium chromate K2CrO4solution?Pb(NO3)2 + K2CrO4 PbCrO4 + 2KNO3[removed] 108 g[removed] 681 g[removed] 639 g[removed] 362 gQuestion 11 (Multiple Choice Worth 2 points)[06.04]On a potential energy diagram for the following processes, which of the following has a decrease in entropy?[removed] ice melts[removed] water freezes[removed] water boils[removed] sublimation of dry ice into carbon dioxide gasQuestion 12 (Multiple Choice Worth 2 points)[07.02]If it requires 37.5 mL of a 0. 245 M HBr solution to neutralize 18.0 mL Mg(OH)2, what is the concentration of the Mg(OH) 2 solution?2 HBr + Mg(OH) 2 Mg(Br) 2 + 2 H2O[removed] 0.0120 M[removed] 0.0255 M[removed] 0.118 M[removed] 0.510 MQuestion 13 (Multiple Choice Worth 2 points)[08.04]What is the purpose of environmental remediation?[removed] to restore water to its original purity levels[removed] to make the most of currently used technologies and resources[removed] to remove pollution or contamination from the environment[removed] to reuse materials that would otherwise go to wasteQuestion 14 (Multiple Choice Worth 2 points)[06.05]According to the collision theory and model created to explain the collision theory, why does a catalyst cause a reaction to speed up?[removed] It lowers the activation energy.[removed] It increases the collisions per minute.[removed] It increases the average kinetic energy of the particles.[removed] It increases the kinetic energy and the collisions per minute.Question 15 (Multiple Choice Worth 2 points)[07.04]What is the correct balanced equation for the following equilibrium constant expression?[removed] CO2 (g) CO (g) + ½ O2 (g)[removed] CO2 (g) CO (g) + O2 (g)[removed] 2 CO2 (g) 2 CO (g) + O2 (g)[removed] 2CO (g) + O2 (g) CO2 (g)Question 16 (Multiple Choice Worth 2 points)[08.03]Which of the following natural resources is considered renewable?[removed] biofuel[removed] natural gas[removed] nuclear power[removed] oilQuestion 17 (Multiple Choice Worth 2 points)[06.05]According to the collision theory and model created to explain the collision theory, what two factors must be satisfied for a given collision to be successful and result in the production of products?[removed] Correct molecular shape and momentum.[removed] Correct position and maximum potential.[removed] Correct density and threshold velocity.[removed] Correct orientation and sufficient energy.Question 18 (Multiple Choice Worth 2 points)[08.02] Which describes nuclear power plants?[removed] They generate power directly from nuclear reactions.[removed] They supply over 50% of the nation’s power needs.[removed] Compared to fossil fuels, they require much less fuel.[removed] They have more atmospheric pollutants compared to fossil fuels.Question 19 (Multiple Choice Worth 2 points)[06.02]When sulfuric acid is poured on sugar the volume expands, it turns black and gets very hot. Which of the following best describes this reaction?[removed] endothermic[removed] exothermic[removed] decomposition[removed] synthesisQuestion 20 (Multiple Choice Worth 2 points)[05.08]Which of the following solutions will have the greatest colligative effect?[removed] 2 moles of glucose (C6H12O6) dissolved in 1.0 kg of water (H2O)[removed] 1.5 moles of sodium chloride (NaCl) dissolved in 1000.0 kg of water (H2O)[removed] 0.75 moles of calcium fluoride (CaF2) dissolved in 500.0 g of water (H2O)[removed] 0.50 moles of carbon dioxide (CO2) dissolved in 250.0 g of water (H2O)Question 21 (Multiple Choice Worth 2 points)[08.06]Biotechnology has allowed us to genetically modify corn with a gene that acts as a pesticide. What could be a possible environmental impact of this development?[removed] Insects resistant to the specific pesticide would develop over time.[removed] The surplus of corn would rot and decay releasing additional greenhouse gases.[removed] The price of corn would drop dramatically because of a greater supply with no increase in demand.[removed] Countries able to buy the new corn seeds would see increases in their economy and pollution would rise.Question 22 (Multiple Choice Worth 2 points)[05.01]Which of the following describes what occurs as a liquid becomes a solid?[removed] A physical change occurs; the particles of the liquid vibrate faster and their kinetic energy increases.[removed] A physical change occurs; the particles of the liquid vibrate more slowly and their kinetic energy decreases.[removed] A chemical change occurs; the particles of the liquid vibrate faster and their kinetic energy increases.[removed] A chemical change occurs; the particles of the liquid vibrate more slowly and their kinetic energy decreases.Question 23 (Multiple Choice Worth 2 points)[05.06]In a body of water, the surface tension caused by the attraction between water molecules is strong. Which of the following is a consequence of this property?[removed] Water is considered to be a universal solvent.[removed] When water freezes, the molecules move farther apart.[removed] Only a limited amount of solute can be dissolved in a sample of water.[removed] Objects with a higher density than water can be observed floating on water.Question 24 (Multiple Choice Worth 2 points)[07.05]What would happen to the following endothermic reaction that is in equilibrium if heat is added?N2O4 (g) 2 NO2 (g)[removed] The reaction would not be affected[removed] The equilibrium would shift to the left[removed] The equilibrium would shift to the right[removed] The product concentration would equal the reactantsQuestion 25 (Multiple Choice Worth 2 points)[05.03]A sample of gas has a volume of 2.4 L and a pressure of 1.2 atm. What would the pressure of the same gas sample be if the volume is reduced to 1.8 L at a constant temperature?[removed] 0.90 atm[removed] 1.6 atm[removed] 5.2 atm[removed] 3.6 atmQuestion 26 (Multiple Choice Worth 2 points)[07.03]Which is not true regarding the pH scale?[removed] The neutral pH at 25°C is 7.0.[removed] Bases have a pH greater than 7.0.[removed] The pH scale measures the hydronium ion concentration in solution.[removed] When the concentration of hydroxide ions increases, the pH decreases.Question 27 (Multiple Choice Worth 2 points)[06.04]Which of the following reactions results in a decrease in entropy?[removed] CaCO3 (s) CaO (s) + CO2 (g)[removed] N2O4 (g) 2NO2 (g)[removed] CaO (s) + SO3 (g) CaSO4 (s)[removed] 2NH3 (g) N2 (g) + 3H2 (g)Question 28 (Multiple Choice Worth 2 points)[07.06]What is the oxidation number of sulfur (S) in sulfuric acid (H2SO4)?[removed] -6[removed] +2[removed] +4[removed] +6Question 29 (Multiple Choice Worth 2 points)[06.04]For an exothermic reaction, which of the following conditions must be true for all products?[removed] The change in enthalpy is positive and potential energy diagram is higher.[removed] The change in enthalpy is negative and potential energy diagram is higher.[removed] The change in enthalpy is positive and potential energy diagram is lower.[removed] The change in enthalpy is negative and potential energy diagram is lower.Question 30 (Multiple Choice Worth 2 points)[05.04]When 7.50 L of sulfur trioxide are produced by the reaction of sulfur dioxide in an excess of oxygen at standard temperature and pressure, how many liters of sulfur dioxide were used?2SO2 (g) + O2 (g) 2SO3 (g)[removed] 3.75 L[removed] 5.00 L[removed] 7.50 L[removed] 15.0 LQuestion 31 (Multiple Choice Worth 2 points)[06.01]If you drop a 150 gram piece of metal that has a temperature of 125°Celsius into 1000 grams of water at 20°Celsius, what best describes what would occur?[removed] More heat will be lost by the metal than gained by the water.[removed] The temperature of the water will be greater than the amount of heat lost by the metal.[removed] The temperature change of the metal will equal the temperature change of the water.[removed] The heat lost by the metal will equal the heat gained by the water.Question 32 (Multiple Choice Worth 2 points)[06.03]Which is not true regarding the specific heat of water?[removed] The specific heat of water explains capillary action.[removed] The specific heat of water is 4.18 J/(°C × g).[removed] Water is useful as an engine coolant because of its high specific heat[removed] The specific heat of water is the reason islands have milder climates.Question 33 (Multiple Choice Worth 2 points)[05.05]Which of the following would be the best technique to use in order to separate a liquid from a solution?[removed] chromatography[removed] evaporation[removed] filtration[removed] simple distillationQuestion 34 (Multiple Choice Worth 2 points)[08.01]Which statement is not correct regarding radiation?[removed] Nuclear reactions arise from an atoms nucleus.[removed] Alpha, Beta, and Gamma are types of radiation.[removed] Most of the earths nuclear energy comes from the Sun.[removed] Radioactive elements have an unbalanced number of protons and electrons.Question 35 (Multiple Choice Worth 2 points)[08.05]Carbon naturally occurs in two forms: diamond and graphite. Why do these two forms have very different properties?[removed] The key difference is that diamonds have other elements bonded within their structure.[removed] The differences are explained by the number of covalent and ionic bonds within each substance.[removed] The differences are explained by the density: graphite is very high and diamond is much lower.[removed] The differences are explained by how the carbon atoms within each substance are covalently bonded together.Question 36 (Multiple Choice Worth 2 points)[05.06]When 5.6 grams of NaCl are dissolved in enough water to create a 125-gram solution, what is the solution’s concentration, expressed as a percent by mass?[removed] 3.6% NaCl[removed] 3.8% NaCl[removed] 4.5% NaCl[removed] 4.7% NaClQuestion 37 (Multiple Choice Worth 2 points)[06.02]On an endothermic potential energy diagram, what is true for all products?[removed] The products are at the same energy level as the reactants.[removed] The products are at a lower energy level than the reactants.[removed] The products are at a higher energy level than the reactants.[removed] The products do not have energy.Question 38 (Multiple Choice Worth 2 points)[06.03]125.0 g of an unknown substance is heated to 97.0°C. It is then placed in a calorimeter than contains 250g of water with an initial temperature of 20.0°C. The final temperature reached by the calorimeter is 23.5°C. What is the specific heat of the unknown substance? The specific heat of water is 4.18 J/ (°C × g).[removed] 0.285 J/ (°C × g)[removed] 0.398 J/ (°C × g)[removed] 0.729 J/ (°C × g)[removed] 1.24 J/ (°C × g)Question 39 (Multiple Choice Worth 2 points)[06.01]How would a system which exchanges energy but does not exchange matter between the system and the surroundings be classified?[removed] an open system[removed] an isolated system[removed] a closed system[removed] an integrated systemQuestion 40 (Multiple Choice Worth 2 points)[07.05]Which of the following is not a result when a change to an equilibrium system is applied?[removed] Increasing the rate of the forward reaction will cause a shift to the left.[removed] Increasing the rate of the reverse reaction will cause a shift to the left.[removed] Decreasing the rate of the forward reaction will cause a shift to the left.[removed] Decreasing the rate of the reverse reaction will cause a shift to the right.Question 41 (Multiple Choice Worth 2 points)[08.04]Which of the following best summarizes the main causes of water pollution today?[removed] increased runoff, driving, discarded oil[removed] evaporation, new construction, overpopulation[removed] waste from wildlife, decaying vegetation, automobiles[removed] leaking septic and sewer systems, manufacturing, farmingQuestion 42 (Multiple Choice Worth 2 points)[08.05]A carbon atom has a strong tendency to do which of the following?[removed] double bond with electrons[removed] receive electrons[removed] donate electrons[removed] share electronsQuestion 43 (Multiple Choice Worth 2 points)[07.01]What is the difference between a strong acid and a weak acid?[removed] A strong acid has a higher pH than a weak acid.[removed] A strong acid is 100% ionized, a weak acid is less than 100% ionized.[removed] A strong acid is diprotic or triprotic, a weak acid is monoprotic.[removed] A strong acid has a greater concentration of hydroxide ions compared to a weak acid.Question 44 (Multiple Choice Worth 2 points)[07.01]Which of the following is not true of acids?[removed] Acids are corrosive.[removed] Dilute acids feel slippery.[removed] Acids have a distinctly sour taste.[removed] Acids have more hydronium ions than hydroxide ionsQuestion 45 (Multiple Choice Worth 2 points)[07.04]Which answer does not describe the following reaction?NO (g) + O2 (g) 2 NO2 (g)[removed] The reaction is in dynamic equilibrium.[removed] The reaction does not go to completion.[removed] The reaction is reversible.[removed] The concentration of reactants and products will be equal.Question 46 (Multiple Choice Worth 2 points)[08.02]How can a sample of uranium-235 that has critical mass be induced to react?[removed] It must be spilt with a laser.[removed] It must be fused to a helium nucleus.[removed] It must be bombarded it with neutrons.[removed] It must be shot with light speed electrons.
