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1. Two systems at different temperatures come in contact. The heat will flow from the system at
A. 30°C to a system at 317 KB. 40°C to a system at 323 KC. 50°C to a system at 303 KD. 60°C to a system at 358 KE. 70°C to a system at 370 K
2. How many joules of heat are released by a 150-gram sample of water that that cools from 25°C to 5°C? (c for H2O is 4.18 J/gK)
A. 78,375 joulesB. 83.6 joulesC. 720 joulesD. 627 joulesE. 12,540 joules
3. Calculate the number of joules required to completely evaporate 18 grams of water at 98°C. (Hv = 2259 J/g and c = 4.18 J/gK)
A. 40,812 joulesB. 40,512 joulesC. 150 joulesD. 40,662 joulesE. 6.12 × 106 joules
4. Which process below has been described correctly for a temperature above 274K?
A. H2O(l) → H2O(s) is exothermic and spontaneous.B. H2O(l) → H2O(s) is endothermic and spontaneous.C. H2O(g) → H2O(l) is endothermic and spontaneous.D. H2O(s) → H2O(l) is endothermic and spontaneous.E. H2O(s) → H2O(l) is exothermic and spontaneous.
5. Based on Gibbs Free Energy equation ΔG =ΔH-TΔS, a process will occur spontaneously when
A. ΔG is positive and ΔS is positiveB. ΔH is positive and ΔT is negativeC. ΔH is negative and ΔS is positiveD. ΔH is negative and ΔS is negativeE. ΔG is positive and ΔS is negative
6. The overall reaction: A + B + 1.5C →D has three individual reactions that take place,
Step 1: A + 2B → EStep 2: F → B + CStep 3: ?What is the reaction that takes place in Step 3?
A. D + F → C + EB. E + 5/2C → D + FC. D + 3/2C → A + ED. B + C → F + EE. A + B + 1.5C → D
7. Calculate the heat for the overall reaction:
Mg(s) + 1/2O2 → MgO(s) given the heats of reaction below:
Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)ΔH = -143 kJMgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(g)ΔH = -216 kJH2(g) + 1 /2O2 → H2O(l)ΔH = -285 kJ
A. -644 kJB. -212 kJC. +644 kJD. -74 kJE. +74 kJ
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