1. Which of the following will have the greatest standard molar entropy (Sº)? a. NH3(g) d....
1. Which of the following is in the correct order of standard state entropy? I. Liquid water < gaseous water II. Liquid water < solid water III. NH; <H3 a. I only b. II only III only d. I and II only e. I and III only c. 2. Which of the following will have the greatest standard molar entropy (Sº)? a. NH3(g) d. H2O(1) b. He(g) CaCO3(s) c. C(s, graphite) e. 3. Indicate which of the following has the...
Short Answer: (4 points each) 1.) Predict whether the entropy change is positive or negative for each of the following reactions. GIVE YOUR REASON FOR YOUR PREDICTIONS a) 2KC1O4(s) → 2KCIO3() + O2(8) b) H2O → H2O) c) 2Na(3) + H2O → 2NaOH(aq) + H2() d) N2(g) → 2N) 2.) State whether the sign of the entropy change expected for each of the following processes will be positive or negative, and EXPLAIN YOUR PREDICTIONS. a) PC130) + Cl2(e) → PCls(s)...
Which system has the greatest entropy? A. 1 mol of H2(g) at STP B. 1 mol of H2(g) at 100∘C 0.5 atm C. 1 mol of H2O(s) at 0∘C D. 1 mol of H2O(l) at 25∘C
For each of the following pairs, indicate which substance possesses the larger standard entropy. Part A 1 mol of P4(g) at 300 ∘C, 0.01 atm, or 1 mol of As4(g) at 300 ∘C, 0.01 atm 1 of at 300 , 0.01 , or 1 of at 300 , 0.01 1 mol of P4(g) at 300 ∘C, 0.01 atm 1 mol of As4(g) at 300 ∘C, 0.01 atm Part B 1 mol of H2O(g) at 100 ∘C, 1 atm, or 1...
17.51 Calculate the entropy change for the following processes. (a) 1.00 mol H,O(s) melts at 0 °C. AH = 6.01 kJ/mol. (b) 2.00 mol CH.() vaporizes at 80.0 °C. AH vap = 30.7 kJ/mol. 17.52 - Calculate the entropy change for the following processes. (a) 2.00 mol NH3(e) vaporizes at -33.0 °C. AHvap = 23.35 kJ/mol. (b) 1.00 mol C,H,OH(s) melts at -114 °C. AHjus = 5.0 kJ/mol. 17.53 Use data from Appendix G to calculate the standard entropy change...
Using the standard entropy values: NOG), S = +210.6 J mol-1 K-1 02(0), sº = +205.0 J mol-1 K-1 NO2(g), sº = +240.5 J mol-1 K-1 calculate the standard entropy change, Asº, for the reaction: NO(g) + O2(g) NO2(g) A.-246.1 kJ B. +246.1 kJ C.-175.1 kJ D.-656.1 kJ E. -72.6 kJ
1. Determine the ∆Sº using Appendix G for the following reaction. C2H5OH(l) + 3 O2(g) --> 2 CO2(g) + 3 H2O(l) Report your answer to three sig figs. Omit unit labels. Only add a - number is the sign is negative. Adding a + to a positive answer messes up the grading. 2. Which of the following equations will have a negative ∆S? A. 3 H2(g)+ N2(g) --> 2 NH3(g) B. C6H6(l)--> C6H6(g) C. NH4OH(s)--> H2O(l)+ NH3(g) D. NaCl(s) -->...
Model - Entropy as a State Function Entropy, S, as with all other state functions like internal energy, E, and enthalpy, H, is a function of the state of a system. Because measuring the absolute state of a system more difficult than measuring the changes in its states, it is the change in entropy, ΔS, in which we will be interested. This means the only aspects that will interest us will be the difference in the final and initial entropies...
The standard cell potential for the fuel cell 2 H2(g) + O2(g) → 2 H2O(l) is E° = +1.23 V at 298 K and +1.18 at 358 K. Estimate the standard entropy change of the cell reaction. Use Table 7.1. to determine v (E-E) A. Sº = vF 7. 0 -160 J mol-1 K-1 0-320 J mol-1 k-1 O-107 J mol-1 K-1 0 -80 J mol-1 k-1
For the reactions below, which reactions have negative entropy? 1. AgNO3(aq) + NaCl(aq) --> AgCl(s) + NaNO3(aq) 2. H2O(g) + CO2(8) --> H2CO3(aq) 3. H2(g) +12(8) --> 2 HI(g) 4. C2H2O2(g) --> 2 CO(g) + H2(g) 5. H2O(g) --> H2O(1) O 2, 3, 4 1, 2,5 1,4,5 0 2,4