Chemistry CP CRT Study Guide Second Quarter 2007-08

Chemistry CP CRT Study Guide Second Quarter 2007-08

Chemistry CP CRT Study Guide Second Quarter 2007-08

This is not the test. This is a guide to the type of question that will appear on the test.

# / AL COS #
#4.0 / What type of solution that contains all of the solute it can hold at a given temperature?
#4.0 / What type of solution that contains less solute than it is able to hold at a given temperature?
#4.0 / What type of solution that contains more solute than it can hold at a given temperature?
#4.0 / What is the term for a solution in which water is the solvent?
#4.0 / If a crystal is added to an aqueous solution and it causes many crystals to come out of the solution, what type of solution was it originally?
#4.0 / What term describes two liquids that can be mixed together but separate shortly after you cease mixing them?
#4.0 / What term describes two liquids that are soluble in each other?
#4.0 / What is the substance that is dissolved in a solution?
#4.0 / What is the substance that dissolves a solute to form a solution?
#4.0 / What explains the solubility of ionic substances in water?
#4.1 / From a graph be able to determine solubility.
#4.1 / Does increasing temperature generally increase the solubility of a solid solute in a solvent?
#4.1 / What is the effect on the rate of solution if the surface area of a solid is increased?
#4.1 / When a gas is dissolved in a liquid, what factor will increase the rate of solution?
#4.1 / What combination of pressure and temperature would increase the solubility of a gas in a liquid?
#4.1 / What factors will speed up the dissolving of a solid solute in water?
#4.1 / A chemist is having some difficulty getting a yellow crystalline solid compound to dissolve in water. What strategies might she employ to increase the solubility of the solid?
#4.1 / A student pours a sample of a clear liquid – whose identify is unknown – into a test tube of water. The water and the liquid form two distinct layers, with the unknown on the bottom. What is true of the system?
#4.3 / What are the products of a neutralization reaction between a strong acid and a strong base?
#4.3 / What type of acids and bases produce only a few ions in solution?
#4.3 / What term refers to the ease with which an acid or base forms ions in solution?
#4.3 / What type of solution contains more hydrogen ions than it does hydroxide ions?
#4.3 / Coffee has a pH of about 5. What type of solution would it form?
#4.3 / What type of solution contains more hydroxide ions than it does hydrogen ions?
#4.3 / What type of acid is nitric acid since it completely ionizes in solution?
#4.3 / What is the negative logarithm of the hydrogen ion concentration known as?
#4.3 / What are the substances produced when KOH (aq) neutralizes HCl (aq) ?
#4.3 / What is the expression that represents the pH of a solution?
#4.3 / Given: H2O, NaOH, HC2H3O2, or CH4, choose the strong base.
#4.3 / What are the products of the neutralization reaction between sodium hydroxide and sulfuric acid?
#4.4 / What is the molarity of a solution made by dissolving 17.0 g of lithium iodide (LiI) in enough water to make 500 mL of solution?
#4.4 / What is the molarity of a solution made by dissolving 34.0 g of sodium chloride (NaCl) in enough water to make 500 mL of solution?
#4.4 / Calculate the molarity of a water solution of CaCl2, given that 5.04 L of the solution contains 612 g of CaCl2.
#4.4 / Calculate the molarity of a water solution of KCl, given that 2.50 L of the solution contains 350 g of KCl.
#4.4 / What would the final volume of a solution be if 25.0 mL of a 1.0 M stock solution is diluted to 0.50 M?
#4.4 / What is the molarity of a solution containing 9.0 moles of a solute in 500.0 mL of solution?
#4.4 / What would the final volume of a solution be if 6.0 mL of a 0.050 M stock solution is diluted to 0.020 M?
#4.4 / What is the molarity of an aqueous solution containing 40.0 g of glucose (C6H12O6) in 1.5 L ofsolution?
#4.4 / What is the molarity of an aqueous solution that contains 14.2 g NaCl dissolved in 2000.0 mL of the solution?
#4.4 / If 40.0 ml of a 0.400 M solution of HCl is diluted to 50.0 ml, what will the final molarity be?
#5.1 / What is a substance that increases the rate of a chemical reaction without being used up?
#5.1 / What is the primary reason an increase in temperature results in an increase in the reaction rate?
#5.1 / What would slow down the rate of a chemical reaction?
#5.1 / What will increase the reaction rate?
#5.1 / What will happen to the rate of reaction if the surface area of reactants is increased?
#5.1 / What will happen to the rate of reaction if the temperature is lowered?
#5.1 / What must occur in order for gas particles to react?
#5.1 / What is the minimum energy required for an effective collision?
#5.1 / What is a substance that slows down chemical processes with out being used up?
#5.1 / From a diagram determine what is the activation energy.
#5.1 / How does a catalyst increases the rate of a chemical reaction?
#6.0 / If 2.50 moles of potassium chlorate are used, how many moles of water would be produced?
8 KClO3 + C12H22O11  8 KCl + 12 CO2 + 11 H2O
#6.0 / How many moles of potassium chlorate are required to produce 18.0 g of water?
8 KClO3 + C12H22O11 8 KCl + 12 CO2 + 11 H2O
#6.0 / If 22.0 g of carbon dioxide are produced, how many grams of sugar (C12H22O11) were used?
8 KClO3 + C12H22O11  8 KCl + 12 CO2 + 11 H2O
#6.0 / How many grams of sugar (C12H22O11) were oxidized by the potassium chlorate, if 3.16 g of water were produced?
8 KClO3 + C12H22O11  8 KCl + 12 CO2 + 11 H2O
#6.0 / Ammonia (NH3) is used to make fertilizer. If you have 1.00 x 10 3g of N2 how many grams of ammonia can be produced?
N2 + 3H2  2NH3
#6.0 / Calculate the number of moles in 350.0g of potassium chlorate (KClO3).
#6.0 / Determine the molar mass of KC2H3O2.
#6.0 / Determine the number of moles in 25.50 g Ag.
#6.0 / Given 3.25 mol of AgNO3, determine the number of formula units.
#6.0 / How many atoms of Cu are in 3.00 moles?
#6.0 / How many grams of CCl4 are in 6.00 moles? The formula mass of carbon tetrachloride is 153.8 g/mol.
#6.0 / How many grams of CH3Br could be made from 10.0 g of CH3OH and excess PBr3?
3 CH3OH + PBr3  3 CH3Br + P(OH)3
#6.0 / How many grams of ZnCl2 are produced from 75.00 g of ZnO in the reaction?
ZnO + 2HCl  ZnCl2 + H2O
#6.0 / How many hydrogen atoms are there in 1.0 x 102 g of glucose, C6H12O6?
#6.0 / How many moles are in 1.2 X 1024 molecules of water?
#6.0 / How many moles of CH3Br could be made from 3.0 moles of PBr3 and excess CH3OH?
3CH3OH + PBr3  3 CH3Br + P(OH)3
#6.0 / In the equation HCl + KOH  KCl + H2O, how many grams of water are produced if 3.00 moles of HCl are used?
#6.0 / In the reaction 2Na + Cl2 2NaCl, how many grams of sodium chloride can be produced from
120.0 g of sodium in the presence of excess chlorine?
#6.0 / One in a series of reactions that inflates airbags in automobiles is the decomposition of sodium azide
(NaN3). 2 NaN3 (s)  2 Na (s) + 3 N2 (g)
Determine the mass of N2 produced if 1.00 x 102 g NaN3 is decomposed.
#6.0 / What is the correct molar mass of Ca(OH)2 ?
#6.0 / What is the formula mass of (NH4)3PO4 ?
#6.0 / The molar mass of CO2 is 44 g/mol. How many moles are present in 110 g?
#6.0 / The molar mass of H2O is 18.015 g/mol. How many moles of water are present in 3.6 g?
#6.0 / The molar mass of NH3 is 17.0 g/mol. How many grams of NH3 are present in 3.50 moles?
#6.0 / What volume of oxygen is needed to completely combust 2.36 L of methane gas (CH4)?
CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (g)
#6.4 / A reaction in which oxygen combines with a substance and releases heat and light can be classified as what type of reaction?
#6.4 / A reaction in which the atoms of one element replace the atoms of another element in a compound can be classified as what type of reaction?
#6.4 / The following reaction : AgNO3(aq) + NaCl (aq) AgCl(s) + NaNO3(aq) , can be classified as what type of reaction?
#6.4 / The following reaction :2Hg + O2 2HgO can be classified as what type of reaction?
#6.4 / Given the following combustion reaction of a hydrocarbon, balance the equation and determine the coefficient of H2O.
C4H6 + O2  CO2 + H2O
#6.4 / What is the coefficient that belongs in front of carbon dioxide in the equation?
____C3H8 + ___O2 ____CO2 + ___H2O
#6.4 / What is the coefficient that belongs in front of oxygen in the equation?
____C3H8 + ___O2 ____CO2 + ___H2O
#6.4 / What is the coefficient that belongs in front of water in the equation?
____C3H8 + ___O2 ____CO2 + ___H2O
#6.4 / What are the coefficients to correctly balance the formula equation?
Al2(SO4)3 + KOH  Al(OH)3 + K2SO4
#6.4 / What are the coefficients to correctly balance the formula equation?
Cr + Fe(NO3)2  Fe + Cr(NO3)3
#6.4 / The following reaction : Cr + Fe(NO3)2  Fe + Cr(NO3)3, can be classified as what type of reaction?
#6.4 / The following reaction : H2O  H2 + O2can be classified as what type of reaction?
#6.4 / What are the coefficients to correctly balance the formula equation?
Pb(NO3)2 (aq) + KI (aq)  PbI2 (s) + KNO3(aq)
#6.4 / What are the coefficients to correctly balance the formula equation?
AlCl3(aq) + Pb(NO3)2(aq)  PbCl2(s) + Al(NO3)3(aq)
#6.4 / What is the balanced equation when aluminum reacts with copper(II)sulfate?
#6.5 / A compound contains 36.1 g calcium and 63.9 g chlorine. What is the empirical formula of the compound?
#6.5 / A compound is composed of 82.68% mercury, (Hg), and 17.32% nitrogen, (N). What is the compound's empirical formula?
#6.5 / Determine the empirical formula for a compound that contains 35.98% aluminum and 64.02 %sulfur.
#6.5 / Find the empirical formula of a compound that is 39.12 % C, 8.76% H, and 52.12% O.
#6.5 / The elemental analysis of a sample of ionic compound gave the following results: 2.82 g Na,
4.35 g Cl, and 7.83 g O. The empirical formula of this compound is:
#6.5 / What is the empirical formula for a compound that is 27.3 % C and 72.7 % O?
#6.5 / What is the molecular formula of a compound that is composed of 83.64% tin (Sn) and 16.36% phosphorous (P)? The compound's experimental molar mass is: 567.80 g/mol.
#6.5 / Find the empirical formula of a compound that is 65.45 % C, 5.45% H, and 29.09% O.
#6.5 / Find the empirical formula of a compound that is 53.5 g C, 15.7 g H, 31.1 g N.
#6.5 / A colorless liquid composed of 46.68% N and 53.32 % O has a molar mass of 60.01 g/mol. Find the molecular formula.
#6.6 / Methane (CH4) contains 75% carbon. What percentage of methane is hydrogen?
#6.6 / Find the percent composition of MgS.
#6.6 / Find the percent composition of CaC2.
#6.6 / Find the percent composition of KClO4.
#6.6 / Find the percent composition of C12H22O11.
#6.6 / Find the percent composition of MgSO4.
#6.6 / What is the percentage of chromium in BaCrO4?
#6.6 / What is the percentage of barium in BaCrO4?
#6.6 / What is the percentage of oxygen in BaCrO4?
#6.6 / What is the percentage of carbon in C7H16?
#7.0 / If the pressure exerted by a gas at 25.0o C in a volume of 0.0440 L is 3.81 atm, how many moles of gas are present? (Hint: R = 0.0821 L-atm/mol-K)
#7.0 / Determine the temperature of 2.49 moles of gas contained in a 2.00L vessel at a pressure of 1.41 atm.
#7.0 / Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
#7.0 / What is the pressure in atmospheres of a 0.108 mole sample of helium gas at a temperature of 20.0C if its volume is 0.505 L?
#7.0 / Determine the Kelvin temperature required for 0.0470 mole of gas to fill a balloon to 1.20 L under 0.988 atm pressure.
#7.0 / A sample of gas at 1.50 atm and 4.0 L is compressed to 2.5 L at a constant temperature. What is the new pressure?
#7.0 / A sample of gas at 313 K occupies a volume of 2.32 L. If the temperature is raised to 348 K what will be the new volume?
#7.0 / You have 422.0 cm3 of nitrogen(IV) oxide at a temperature of 295.15 K and a pressure of 101.325 kPa. What volume will the NO2 occupy at 155.00 kPa and 317.15 K?
#7.0 / A container of gas at 760.0 mm Hg and 20.0C is heated to 40.0C. What is the new pressure in mm Hg?
#7.0 / A gas at 740.0 mm Hg pressure at 25.0 C is cooled to –10.0 C. What is the final pressure in mm Hg?
#7.0 / What is the final pressure in atm, if 10.0 L of gas at 25.0C and 1.00 atm pressure is compressed to 2.00 L at 323C?
#7.0 / What pressure will be needed to reduce the volume of 77.4 L of helium at 98.0 kPa to a volume of 60.0L?
#7.0 / A sample of SO2 gas has a volume of 1.16 L at a temperature of 23o C. At what temperature will the gas have a volume of 1.25 L?
#7.0 / A sample of ammonia gas occupies a volume of 1.58 L at 22.0o C and a pressure of 0.983 atm. What volume will the sample occupy at 1.00 atm and 0 oC?
#7.0 / A student collects 285 mL of O2 gas at a temperature of 15.0C and a pressure of 99.9 kPa. The next day the sample occupies 292 mL at a temperature of 11.0o C. What is the new pressure of the gas?
#7.0 / A sample of gas at 2.50 atm and 6.50 L is compressed to 1.50L at a constant temperature. What is the new pressure?
#7.0 / A sample of gas at 255 K occupies a volume of 1.55 L. If the temperature is raised to 298 K what will be the new volume?
#7.0 / You have 200.0 cm3 of nitrogen (IV) oxide at a temperature of 303.0 K and a pressure of 101.0 kPa. What volume will the NO2 occupy at 255.0 kPa and 371.0 K?
#7.0 / A container of gas at 550.0 mm Hg and 35.0C is heated to 60.0C. What is the new pressure in mm Hg?
#7.0 / A gas at 925.0 mm Hg pressure at 50.00 C is cooled to –25.00 C. What is the final pressure in mm Hg?
#7.0 / What is the final pressure in atm, if 5.25 L of gas at 75.0C and 1.33 atm pressure is compressed to 2.75 L at 155 C?
#7.0 / What pressure will be needed to change the volume of 22.4 L of helium at 25.0 kPa to a volume of 85.0L?
#7.0 / A sample of SO2 gas has a volume of 9.50 L at a temperature of 320K. At what temperature will the gas have a volume of 2.55 L?
#7.0 / A sample of ammonia gas occupies a volume of 27.4 L at 14.0o C and a pressure of 1.20 atm. What volume will the sample occupy at 3.00 atm and 0 oC?
#7.0 / A student collects 355 mL of O2 gas at a temperature of 27C and a pressure of 127 kPa. The next day the sample occupies 257 mL at a temperature of 17o C, What is the new pressure of the gas?
#8.1 / What type of reactions occurs when more energy is released in the forming of new bonds than is required to break bonds in the initial reactants?
#8.1 / What type of reactions occurs when more energy is required to break existing bonds in reactants than is released when new bonds form in the products?
#8.1 / What type of reactions release energy into its surroundings?
#8.1 / What type of energy change is shown in the following reaction
Sn +Cl2 SnCl2 H= -325KJ
#8.1 / A 50.6 g sample of iron metal is heated from 19.7o C to 24.3o C. How many joules of heat will be absorbed? (specific heat of iron is 0.4494(J/g oC)
#8.1 / A sample of an unknown metal has a mass of 120.7 g. As the sample cools from 90.5oC to 25.7oC, it releases 7020 J of energy. What is the specific heat of the sample?
#8.1 / A silver bar with a mass of 250.0 g is heated from 22.0 oC to 68.5 oC. How much heat does the silver bar absorb? The specific heat of silver is 0.235 J/g.oC.
#8.1 / If the temperature of 34.4 g of ethanol increases from 25.0o C to 78.8o C, how much heat has been absorbed by the ethanol? (The specific heat of ethanol is 2.44 J/g- oC).
#8.1 / The temperature of a sample of iron with a mass of 10.0 g changed from 50.4C to 25.0C with the release of 114 J of heat. What is the specific heat of iron?
#8.1 / The specific heat of ethanol is 2.44 J/gC. How many joules of energy are required to heat 50.0 g of ethanol from -20.0C to 68.0C?
#8.1 / How much heat does it take to warm 16.0 g of pure water from 90C to 100 C? The specific heat of water is 4.18 J/gC.
#8.1 / How much heat does it take to warm 50.00 g of pure water from 20.00C to 80.00 C? The specific heat of water is 4.180 J/gC.
#8.1 / If the temperature of 56.2 g of ethanol increases from 75.1o C to 89.3o C, how much heat has been absorbed by the ethanol? (The specific heat of ethanol is 2.44 J/g- oC).
#8.1 / The temperature of a sample of water increases from 20.0C to 46.6C as it absorbs 5650 J of heat. What is the mass of the sample? The specific heat of water is 4.18 J/gC.
#8.1 / From a graph be able to determine if a reaction is endothermic or exothermic and why.

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