If a student decreased the temperature for this reaction: C₂H4(g) + H₂(g) - heat C₂H6(g) what would happen? E.. The [C₂H4] would decrease O A, D and E only A & D only D. The [C₂H6] would increase C. The [H₂] would increase OA. The system would shift to the right OB. The system would shift to the left OB & C only

If a student decreased the temperature for this reaction: C₂H4(g) + H₂(g) - heat C₂H6(g) what would happen? E.. The [C₂H4] would decrease O A, D and E only A & D only D. The [C₂H6] would increase C. The [H₂] would increase OA. The system would shift to the right OB. The system would shift to the left OB & C only

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter10: Entropy And The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 10.27PAE: One statement of the second law of thermodynamics is that heat cannot be turned completely into...

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9.96 Most first aid "cold packs" are based on the endothermic dissolution of ammonium nitrate in water: NH4NO3(s)NH4+(aq)+NO3(aq) H= 25.69 kJ A particular cold pack contains 50.0 g of NH4NO3 and 125.0 g of water. When the pack is squeezed, the NH4NO3dissolves in the water. If the pack and its contents are initially at 24.0°C, what is the lowest temperature that this bag could reach? (Assume that the ammonium nitrate solution has a specific heat of 4.25J g-l K-l, and that the heat capacity of the bag itself is small enough to be neglected.)
Consider the system shown in Figure 16.9. What is the change in entropy for the process where the energy is initially associated with particles A and B, and the energy is distributed between two particles in different boxes (one in A-B, the other in C-D)?
What determines Ssurr for a process? To calculate Ssurr at constant pressure and temperature, we use the following equation: Ssurr = H/T. Why does a minus sign appear in the equation, and why is Ssurr inversely proportional to temperature?
Given the following information at 25C, calculate G at 25C for the reaction 2A(g)+B(g)3C(g) Substance Hf(kJ/mol) S(J/molK) A(g) 191 244 B(g) 70.8 300 C(g) 197 164 a 956 kJ b 956 kJ c 346 kJ d 346 kJ e 1.03 103 kJ
9.83 A student performing a calorimetry experiment combined 100.0 mL of 0.50 M HCl and 100.0 mL of 0.50 M NaOH in a coffee cup calorimeter. Both solutions were initially at 20.0°C, but when the two were mixed, the temperature rose to 23.2°C. (a) Suppose the experiment is repeated in the same calorimeter but this time using 200 mL of 0.50 M HCl and 200.0 mL of 0.50 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why? (b) Suppose that the experiment is repeated once again in the same calorimeter, this time using 100 mL of 1.00 M HCl and 100.0 mL of 1.00 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why?
Consider the reaction H2(g)+Br2(g)2HBr(g) where H = 103.8 kJ/mol. In a particular experiment, equal moles of H2(g) at 1.00 atm and Br2(g) at 1.00 atm were mixed in a 1.00-L flask at 25C and allowed to reach equilibrium. Then the molecules of H2 at equilibrium were counted using a very sensitive technique, and 1.10 1013 molecules were found. For this reaction, calculate the values of K, G, and S.
One statement of the second law of thermodynamics is that heat cannot be turned completely into work. Another is that the entropy of the universe always increases. How are these two statements related?
Some water is placed in a coffee-cup calorimeter. When 1.0 g of an ionic solid is added, the temperature of the solution increases from 21.5C to 24.2C as the solid dissolves. For the dissolving process, what are the signs for Ssys, Ssurr, and Suniv?
Why is it usually easier to use G to determine the spontaneity of a process rather than Su ?
How does the second law of thermodynamics explain a spontaneous change in a system that becomes more ordered when that process is exothermic?
9.20 State the first law of thermodynamics briefly in your own words.
Determine whether each of the following statements is true or false. If false, modify to make the statement true. (a) An exothermic reaction is spontaneous. (b) When G is positive, the reaction cannot occur under any conditions. (c) S is positive for a reaction in which there is an increase in the number of moles. (d) If H and S are both negative, G will he negative.