Energetics (Triple) quiz Loading... 1. In an endothermic reaction, which is greater: the energy taken in when breaking bonds or the energy released when bonds are made?Energy taken in when making bondsDepends on the temperature of the surroundingsEnergy taken in when breaking bondsEnergy released when bonds are madeQuestion 1 of 16 Loading... 2. Explain, in terms of making and breaking bonds, why a reaction could be exothermicThe energy needed to break the bonds is more than the energy released to make the bondsThe bonds in the reagents are stronger than the bonds in the productsBreaking the bonds is less favourable than making themThe energy needed to break the bonds is less than the energy released to make the bondsQuestion 2 of 16 Loading... 3. When a solid dissolves, is this process exothermic or endothermic?Depends on the temperature of the surroundingsExothermicDepends on the reagentsEndothermicQuestion 3 of 16 Loading... 4. Use Q=mcΔT and c=4.18J/°C/g. A strip of magnesium is added to a beaker with 200cm³ of copper (II) sulfate. The temperature starts at 21.7°C and rises to a maximum of 23.1°C. What is the total heat energy change?2.153 kJ1247 J1944 kJ1170 JQuestion 4 of 16 Loading... 5. State the units of molar enthalpy change.kJ/molmol/⁰CJ/⁰C/molkJ/⁰CQuestion 5 of 16 Loading... 6. In a combustion calorimetry experiment, 0.78g of ethanol (C₂H₅OH) produced 12,540 J of heat energy. Calculate the molar enthalpy change.-369 kJ/mol (Amount = 0.78/23 = 0.034 mol. Answer = 12540/1000/0.034 = 369 kJ/mol)-213 kJ/mol (Amount = 46/0.78 = 59.0 mol. Answer = 12540/59.0 = 213 kJ/mol)-738 kJ/mol (Amount = 0.78/46 = 0.017 mol. Answer = 12540/1000/0.017 = 738 kJ/mol)-425 kJ/mol (Amount = 23/0.78 = 29.5 mol. Answer = 12540/29.5 = 425 kJ/mol)Question 6 of 16 Loading... 7. Use Q=mcΔT and c=4.18J/°C/g. 25cm³ of sulfuric acid is put into a boiling tube. The starting temperature is 21°C. A spatula of iron filings is added. After a while the temperature reaches 33°C. What is the total heat energy change?1254 J3383 J2.153 kJ2153 JQuestion 7 of 16 Loading... 8. In a calorimetry experiment to investigate the heat energy released by the combustion of ethanol, why should the water in the calorimeter be stirred?To ensure the container does not get too hotTo ensure the heat energy is mixed evenly throughout all the waterTo prevent the water from evaporatingTo allow the heat to spread evenly through the copper containerQuestion 8 of 16 Loading... 9. In a chemical reaction, the overall molar enthalpy is -87 kJ/mol. Is this reaction exothermic or endothermic?Depends on the reagentsDepends on the temperature of the surroundingsExothermicEndothermicQuestion 9 of 16 Loading... 10. What does this diagram represent?Energy level diagram for an exothermic reactionReaction profile for an endothermic reactionEnergy level diagram for an endothermic reactionReaction profile for an exothermic reactionQuestion 10 of 16 Loading... 11. What is meant by the term endothermic?A reaction which will only be spontaneous at cold temperatures (below 0⁰C)A reaction which will only be spontaneous at warm temperatures (above 100⁰C)A reaction in which heat energy is taken in (surroundings get colder)A reaction in which heat energy is given out (surroundings get hotter)Question 11 of 16 Loading... 12. What is meant by the term exothermic?A reaction which will only be spontaneous at warm temperatures (above 100⁰C)A reaction in which heat energy is given out (surroundings get hotter)A reaction in which heat energy is taken in (surroundings get colder)A reaction which will only be spontaneous at cold temperatures (below 0⁰C)Question 12 of 16 Loading... 13. What does the symbol ΔH meanexothermicenthalpy (energy) changeheat energyspecific heat capacityQuestion 13 of 16 Loading... 14. Are displacement reactions exothermic or endothermic?ExothermicDepends on the temperature of the surroundingsEndothermicDepends on the reagentsQuestion 14 of 16 Loading... 15. Explain why experimental values of enthalpy change differ from theoretical valuesDifferent equipment produces different results. Not all the reactants are used upDifferent equipment produces different results. Heat energy is lost to the surroundings. Not all the reactants are used upHeat energy is lost to the surroundings. Not all the reactants are used up.Different equipment produces different results. Heat energy is lost to the surroundingsQuestion 15 of 16 Loading... 16. In a chemical reaction, 250 kJ/mol is taken to break all the bonds and 280 kJ/mol is released when new bonds are formed. What is the overall molar enthalpy of the reaction?+530 kJ/mol-30 kJ/mol+30 kJ/mol-530 kJ/molQuestion 16 of 16 Loading... Related Posts:The entire quiz question bank!The entire quiz question bank (Double only)!Key Calculations quizEquilibria (triple) quizCondensation Polymers quizElectrolysis quiz Hydr0Gen2020-02-16T16:59:30+00:00Categories: Uncategorized|Tags: Quiz, Topic: Energetics| Share This Story, Choose Your Platform! FacebookXRedditLinkedInTumblrPinterestVkEmail