Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Change During an exothermic chemical reaction, a solid is consumed and a gas produced. An endothermic chemical reaction between two liquids results in gaseous products. A gas expands without absorbing or releasing heat. Is this change spontaneous? O Yes. O No. O Can't decide with information given. O Yes. O No. O Can't decide with information given. Yes. No. O Can't decide with information given.

Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Change During an exothermic chemical reaction, a solid is consumed and a gas produced. An endothermic chemical reaction between two liquids results in gaseous products. A gas expands without absorbing or releasing heat. Is this change spontaneous? O Yes. O No. O Can't decide with information given. O Yes. O No. O Can't decide with information given. Yes. No. O Can't decide with information given.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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In the past, scientists were surprised that an endothermic process like the one in this lab, could be spontaneous. Which statement correctly describes why it seems like an endothermic process should not be spontaneous? Group of answer choices All endothermic processes create order in both the system and surroundings. Endothermic processes cause heat to flow from a cold object to a hot object. A process that spontaneously takes in energy seems to be analogous to a rock rolling up a hill. Endothermic processes become so cold that molecular motion stops.
What is the change in enthalpy (∆H) for a chemical reaction?How is ∆H different from ∆E?
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A chemist measures the energy change AH during the following reaction: 2 HgO(s) → 2 Hg(1)+O,(g) AH=182. kJ Use the information to answer the following questions. endothermic. This reaction is... x10 exothermic. Yes, absorbed. Suppose 56.6g of HgO react. Yes, released. Will any heat be released or absorbed? No. If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. kJ Round your answer to 3 significant digits.
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A 2 mole sample of gas expands from a volume of 4 L to 10 L under a constant pressure of 12.5 atm before then dropping to a pressure of 5 atm (while remaining at 10 L). 2 moles of gas expands from a volume of 4L to 10 L under a constant temperature (300K). Which situation requires more work? Why?
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In a reaction similar to Reaction 1, 3.2 g of sodium hydroxide (NaOH) is added to 100.0 g of water. A rise in temperature of 2.9 °C was noted. Assume the solution formed is water and c= 4.184 J/ (g °C). a. Calculate the heat, q, evolved for this reaction. b. How many moles of NaOH were reacted? c. Using the answers to a and b, what is the H for this reaction in kJ/mol?
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