1) Classify if this is Endothermic or HEAT MUST BE ADDED TO Exothermic: GET THE REACTION TO GO. Focus on the reaction. Endothermic Exothermic 2) Classify if this is Endothermic or Exothermic: THE TEMPERATURE OF THE SURROUNDINGS DECREASES. Focus on the surroundings. Endothermic O Exothermic 3) Classify if this is Endothermic or Exothermic: THE POTENTIAL ENERGY OF THE REACTANTS IS GREATER THAN THAT OF THE SURROUNDINGS. Focus on the reactants. Endothermic Exothermic

1) Classify if this is Endothermic or HEAT MUST BE ADDED TO Exothermic: GET THE REACTION TO GO. Focus on the reaction. Endothermic Exothermic 2) Classify if this is Endothermic or Exothermic: THE TEMPERATURE OF THE SURROUNDINGS DECREASES. Focus on the surroundings. Endothermic O Exothermic 3) Classify if this is Endothermic or Exothermic: THE POTENTIAL ENERGY OF THE REACTANTS IS GREATER THAN THAT OF THE SURROUNDINGS. Focus on the reactants. Endothermic Exothermic

Chemistry In Focus

7th Edition

ISBN:9781337399692

Author:Tro, Nivaldo J.

Publisher:Tro, Nivaldo J.

Chapter9: Energy For Today

Section: Chapter Questions

Problem 5SC: When two solutions are mixed in a beaker, a reaction occurs, and the temperature drops. Is the...

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9.58 For the reaction C2H2(g)+2H2(g)C2H6,H=136 kJ. What are the ratios that can be defined between moles of substances and energy?
Enthalpy a A 100.-g sample of water is placed in an insulated container and allowed to come to room temperature at 21C. To heat the water sample to 41C, how much heat must you add to it? b Consider the hypothetical reaction,2X(aq)+Y(l)X2Y(aq)being run in an insulated container that contains 100. g of solution. If the temperature of the solution changes from 21C to 31C, how much heat does the chemical reaction produce? How does this answer compare with that in part a? (You can assume that this solution is so dilute that it has the same heat capacity as pure water.) c If you wanted the temperature of 100. g of this solution to increase from 21C to 51C, how much heat would you have to add to it? (Try to answer this question without using a formula.) d If you had added 0.02 mol of X and 0.01 mol of Y to form the solution in part b, how many moles of X and Y would you need to bring about the temperature change described in part c. e Judging on the basis of your answers so far, what is the enthalpy of the reaction 2X(aq) + Y(l) X2Y(aq)?
For the reaction HgO(s)Hg(l)+12O2(g),H=+90.7kJ: a.What quantity of heat is required to produce 1 mole of mercury by this reaction? b.What quantity of heat is required to produce 1 mole of oxygen gas by this reaction? c.What quantity of heat would be released in the following reaction as written? 2Hg(l) + O2(g) 2HgO(s)
Use Table 8.3 to obtain AHO for the following thermochemical equations: (a) Mg(OH)2(s)+2NH4+(aq)Mg2+(aq)+2NH3(g)+2H2O(l) (b) PbO(s)+C(s)CO(g)+Pb(s) (c) Mn(s)+4 H+(aq)+SO42 Mn2+(aq)+SO2(g)+2H2O(l)
For the reaction HgO(s)Hg(l)+12O2(g),H=+90.7KJ: a. What quantity of heat is required to produce 1 mole of mercury by this reaction? b. What quantity of heat is required to produce 1 mole of oxygen gas by this reaction? c. What quantity of heat would be released in the following reaction as written? 2Hg(l)+O2(g)2HgO(s)
Hypothetical elements A2 and B2 react according to the following equation, forming the compound AB. A2(aq)+B2(aq)2AB(aq);H=+271kJ/mol If solutions A2(aq) and B2(aq), starting at the same temperature, are mixed in a coffee-cup calorimeter, the reaction that occurs is a exothermic, and the temperature of the resulting solution rises. b endothermic, and the temperature of the resulting solution rises. c endothermic, and the temperature of the resulting solution falls. d exothermic, and the temperature of the resulting solution falls. e exothermic or endothermic, depending on the original and final temperatures.
An exothermic reaction is carried out in a coffee-cup calorimeter. Which of the following statements is/are NOT true for the process? (a) The temperature of the water increases. (b) Heat is absorbed by the water. (c) The enthalpy of the products is higher than the enthalpy of the reactants. (d) qH2o=qrxn (e) qrxn0 (f) qrxn+qH2o=0
Determine whether the statements given below are true or false. Consider an endothermic process taking place in a beaker at room temperature. (a) Heat flows from the surroundings to the system. (b) The beaker is cold to the touch. (c) The pressure of the system decreases. (d) The value of q for the system is positive.
Suppose heat flows into a vessel containing a gas. As the heat flows into the gas, what happens to the gas molecules? What happens to the internal energy of the gas?
The enthalpy change for the reaction CH4(g)+2O2(g)CO2(g)+2H2O(l) is 891 kJ for the reaction as written. a. What quantity of heat is released for each mole of water formed? b. What quantity of heat is released for each mole of oxygen reacted?
9.89 A sample of gas is 80.0% CH4 and 20.0% C2H6 by mass. What is the heat from the combustion of 1.00 g of this mixture? Assume the products are CO2 (g) and H2O (l).
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the experimenter used a calorimeter that was a poorer insulator than a coffee cup calorimeter? Explain your answer.

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