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chem exam 4
| Question | Answer |
|---|---|
| An_________ is any compound that can form ions when dissolved in water and therefore conduct electricity. Acids, bases, and soluble salts fit this categoy | electrolye |
| Which of the following situations is most favorable for solubility? Astrong attraction between solute particles B strong attraction between solvent particles C strong attraction of solute particles to solvent particles | C |
| Which of the following would you least expect to find in CaCl2(aq)? A. H2O molecules B. CaCl2 molecules C. Ca2+ ions D. Cl− ions | B. CaCl2 molecules |
| A 0.100 M solution of K2SO4 would contain the same total ion concentration as which of the following solutions? A) 0.0800 MNa2CO3 B) 0.100 MNaCl C) 0.0750 MNa3PO4 D) 0.0500 MNaOH | C. 0.0750 M Na3PO4 |
| Suppose that aqueous solutions of barium nitrate and potassium carbonate are mixed. What is the name of the compound or compounds that precipitate? | barium carbonate |
| Write the ions present in a solution of Na2CO3. | 2Na+, CO32− |
| What is the name of the acid whose formula is HI? | hydroiodic acid |
| What is the formula for chlorous acid? | HClO2 |
| What is the name of the acid whose formula is H2CO3? | carbonic acid |
| What is the formula for sulfurous acid? | H2SO3 |
| An_______ is a compound that can donate H+. You can recognize acid formulas as those that start with H or end with COOH. | acid |
| A______ is a compound that can accept H+. Base formulas often contain a metal cation with the hydroxide anion, OH−. Bases that do not contain OH usually contain N. | base |
| A_____ is an ionic compound that is neither an acid nor a base. To identify a salt, look for a formula that contains a cation that is not H+ and an anion that is not OH−. | salt |
| Name each acid. HIO3(aq) | iodic acid |
| Name each acid. HClO3(aq | chloric acid |
| Name each acid. H2CrO4(aq) | chromic acid |
| What is the name of the base that has the formula Ca(OH)2? | calcium hydroxide |
| What is the chemical formula for the base rubidium hydroxide? | RbOH |
| Which of these compounds is not a base? A) CsOH B) C2H5NH2 C) Fe(OH)2 D) HF | HF |
| In_________ reactions a solid product forms from aqueous reactants. The product can be predicted by using solubility rules. | precipitation |
| In ______________ reactions an acid (proton donor) reacts with a base (proton acceptor) to form an ionic salt and sometimes water. You can recognize this type of reaction by the presence of an acid and base in the reactants. | acid-base neutralization |
| In__________reactions electrons are transferred between reactants. So you will always see changes in oxidation number within this type of reaction. | oxidation-reduction |
| An _______ ________t is an element or compound in a redox reaction that oxidizes another species and itself gets reduced and is therefore the electron acceptor in the reaction. | oxidizing agen |
| A _______ _______is an element or compound in a redox reaction that reduces another species and itself gets oxidized and is therefore the electron donor in the reaction. | reducing agent |
| Which element is oxidized in this reaction? Fe2O3+3CO→ 2Fe+3CO2 | carbon |
| Which substance is the oxidizing agent in this reaction? Fe2O3+3CO→ 2Fe+3CO2 | Fe2O3 |
| Which element is reduced in this reaction? Cr2O72−+3HNO2+5H+→ 2Cr3++3NO3−+4H2O | Cr |
| Which substance is the reducing agent in this reaction? Cr2O72−+3HNO2+5H+→ 2Cr3++3NO3−+4H2O | HNO2 |
| In most cases, oxygen has an oxidation state of ______. Group 1 and group 2 elements on the periodic table have ___ and ____ oxidation states, respectively. In most cases, hydrogen has an oxidation state of ____. | −2; +1 and +2; +1 |
| work is = _____ x _______ | force x distance |
| (kg m^2)/s^2 = | joule |
| positive energy = ________ | repulsion |
| negative energy = _______ | attractive |
| energy is conserved; energy is constant | first law of thermodynamics |
| energy = ______ energy + _______ energy | potential; kinetic |
| change in energy = energy of ______ - energy of _______ | products; reactants |
| if the energy of the products is greater than the reactants, energy goes ________ systems | into (positive energy) |
| if energy of the products is less than energy of reactants, energy goes ________ systems | out of (negative energy) |
| the change in energy = ____ + ____ | q+ w (heat plus work) |
| when q is +, energy flows ______ system when q is - , energy flows ______ system | into; out of |
| when w is +,, work on ________ when w is - , work on ______ | system - contracting surroundings - increase volume |
| heat flows from _____ to _____ | hot; cold |
| temperature increases aas a function of _____ _____ | heat capacity |
| energy required to raise the emperature of an object by 1 degree celsius | heat capacity |
| heat capacity per mole of substance | molar heat capacity |
| heat capacity per gram of substance | specific heat |
| specific heat = | energy (J)/ (g * K) |
| work= -P(change in volume) what are the units? | L * atm |
| in constant volume calorimetry, ___=0 since volume is = 0 | work |
| in constant volume calorimetry, heat of the reaction (q)= __________ | - heat of the calorimeter |
| in constant volume calorimetry, the change in energy = (________)/(_______) | (heat of the reaction)/(moles of compound) |
| when q is +, heat goes_______ the reaction when q is -, heat goes_____ of the reaction | into; out |
| when q is +, there is a ____ delta H, meaning it is ______ when q is -, there is a ____ delta H, meaning it is ______ | positive; endothermic negative; exothermic |
| the heat of the solution is = multiplying what 3 things heat of reaction = - heat of solution | SH (mass) (change in T) |
| delta H units | kJ/mole |
| standard states for standard enthalpy of formation for gas = liquids, solids = solutions | 1 atm pressure most stable phase at 25 C, 1 atm 1 M solution |
| formation of 1 mole of product from constituent elements | enthalpy |
| the standard enthalpy of formation for any reaction is | sum of the products times stoichimetric coefficients - sum of reactants and stoichometric |
| standard enthalpy of formation for pure elemtns | 0 |
| the change in enthalpy for a reaction can also be determined by the sum of bonds _________ - the sum of bonds __________ | breaking; forming |
| for lattice energy, as charge increases, lattice energy _________. as distance decreases, lattice energy __________ | increases; decreases |
| heat per gram of fuel | fuel value |
| Compounds of group ____ions are soluble. _______ and _________s are soluble. Except for the compounds covered by rule 1, ______,_______,_______,________ are insoluble. | I ; Nitrates and chlorate; carbonates, hydroxides, phosphates, and sulfides |
| in naming acids ate changes to____ (retain prefixes) and ite changes to _____ (retain prefixes). | ic; ous |
| when finding the oxidation number for an individual atom in a diatomic atom (C2) MAKE SURE YOU FIND IT THEN DIVIDE BY THE SUBSCRIPT! | |
| #1 ch 10 | |
| A mole of X reacts at a constant pressure of 43.0 atm via the reaction X(g)+4Y(g)→2Z(g), ΔH∘=−75.0 kJ Before the reaction, the volume of the gaseous mixture was 5.00 L. After the reaction, the volume was 2.00 L. Calculate the , ΔE, in kilojoules. | -62 kJ |
| # 2 ch 10 part A | |
| A piston has an external pressure of 9.00 atm. How much work has been done in joules if the cylinder goes from a volume of 0.140 liters to 0.650 liters? | w = -465 J |
| 1 N * m (force x distance) = 1 ________ | joule |
| heat or work? a. A rolling billiard ball collides with another billiard ball. The first billiard ball (defined as the system) stops rolling after the collision. what is the sign of delta E? | work ; negative |
| heat or work? b. A book is dropped to the floor (the book is the system). what is the sign of delta E? | work ; negtive |
| heat or work? c. A father pushes his daughter on a swing (the daughter and the swing are the system). what is the sign of delta E? | work ; positive |
| The air in an inflated balloon (defined as the system) is warmed over a toaster and absorbs 110 J of heat. As it expands, it does 79 kJ of work.What is the change in internal energy for the system? | -79 kJ |
| It takes 47.0 J to raise the temperature of an 10.8 g piece of unknown metal from 13.0∘C to 24.9 ∘C. What is the specific heat for the metal? | .366 J/g*C |
| The molar heat capacity of silver is 25.35 J/mol⋅∘C. How much energy would it take to raise the temperature of 10.8 g of silver by 19.5 ∘C? | 49.4 J |
| What is the specific heat of silver? | .235 J/ g*C |
| How much heat is required to warm 1.30 kg of sand from 30.0 ∘C to 100.0 ∘C? | 7.64 * 10 ^4 J |
| A volume of 115 mL of H2O is initially at room temperature (22.00 ∘C). A chilled steel rod at 2.00 ∘C is placed in the water. If the final temperature of the system is 21.50 ∘C , what is the mass of the steel bar? SH water - 4.184; SH steel = .452 | 27. 3 g |
| The specific heat of water is 4.18 J/(g⋅∘C). Calculate the molar heat capacity of water | 75.2 |
| #9 ch 10 | |
| Determine whether each of the preceding is exothermic or endothermic and Indicate the sign of ΔH.. a. dry ice evaporating b. a sparkler burning c. the reaction that occurs in a chemical cold pack often used to ice athletic injuries | a. endothermic - positive b. exothermic - negative c. endothermic - positive |
| What mass of natural gas (CH4) must you burn to emit 263 kJ of heat? CH4(g)+2O2(g)→ CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ | 5.26 g |
| A total of 2.00 mol of a compound is allowed to react with water in a foam coffee cup and the reaction produces 189 g of solution. The reaction caused the temperature of the solution to rise from 21.00 to 24.70 ∘C. What is the enthalpy of this reaction? | -1.46 kJ/mol |
| #13 ch 10 | |
| A 32.9 g iron rod, initially at 22.7 ∘C, is submerged into an unknown mass of water at 63.4 ∘C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 59.0 ∘C. mass of water? | 29 g |
| #15, #16 ch 10 | |
| C3H8(g)+5O2(g)→3CO2(g)+4H2O(g). Calculate ΔH∘rxn for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of gaseous propane is -103.9 kJ/mol.) | -2043. 8 kJ |
| #18 ch 10 | |
| When NH4ClO4(s) decomposes thermally, the products of the reaction are N2(g), O2(g), H2O(g), and HCl(g). Write the balanced equation (including phases) for this reaction. | 4NH4ClO4(s)→ 2N2(g)+5O2(g)+6H2O(g)+4HC |
| #19 ch 10 | |
| #20 ch 10 | |
| microwave radiation has wavelength of 11.2 cm . How many photons are required to heat 245 mL of coffee from 25.0 ∘C to 62.0 ∘C? Assume that the coffee has the same density, and specific heat capacity,as water over this temperature range. | 2.13 * 10^28 photons |
| H2O(l)→H2O(g) ΔH∘rxn=+44.01kJ. Estimate the mass of water that must evaporate from the skin to cool the body by 0.50 ∘C. Assume a body mass of 95 kg and assume that the specific heat capacity of the body is 4.0 J/g⋅∘C. | 78 g |
| C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) ΔH∘rxn=−2044kJ. What mass of LP gas is necessary to heat 1.3 L of water from room temperature (25.0 ∘C) to boiling (100.0 ∘C)? 16% of the heat emitted by the LP gas combustion goes to heat the water | 55 g |
| Rank the following ionic compounds by the magnitude of their lattice energy.Na2O Na2S MgO LiCl BeO | highest to lowest: BeO, MgO, Na2O, Na2S, LiCl |
| #24 ch 10 part 2 | |
| Arrange the following substances in order of decreasing magnitude of lattice energy. CaO MgO KCl NaF | MgO, CaO, NaF, KCl |
| Write a balanced equation for the complete combustion of palmitic acid. Use H2O(l) in the balanced chemical equation because the metabolism of these compounds produces liquid water. | C16H32O2(s)+23O2(g)→ 16CO2(g)+16H2O(l) |
| Calculate the standard enthalpy of combustion. The standard enthalpy of formation of palmitic acid - 208kJ/mol. | −1.066×104 kJ |
| What is the caloric content of palmitic acid in Cal/g? | 9.938 Cal/ g |
| Write a balanced equation for the complete combustion of table sugar (sucrose, C12H22O11). Use H2O(l) in the balanced chemical equation because the metabolism of these compounds produces liquid water. | C12H22O11(s)+12O2(g)→ 12CO2(g)+11H2O |
| Calculate the standard enthalpy of combustion. The standard enthalpy of formation of sucrose is - 2226.1kJ/mol. | -5640 |
| What is the caloric content of sucrose in Cal/g? | 3.938 Cal/ g |
| One tablespoon of peanut butter has a mass of 17 g . It is combusted in a calorimeter whose heat capacity is 120 kJ/∘C . The temperature of the calorimeter rises from 22.5 ∘C to 25.5 ∘C.Find the food caloric content of peanut butter. | 5.1 Cal/ g |
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jackjack109