Question 10 2 pts Select ALL the reaction(s) that is/are most likely to have a positive...
3 3 points Which reaction, shown below, is most likely to have a positive entropy (S) of the system? O SiO2 (s) + 3C (s) --> SIC(s) + 2CO (g) O 6CO2 (g) + 6H20 (1) --> C6H12O6 (s) + 602 (g) O CO(g) + Cl2 (g) --> COCI2 (g) 03NO2 (g) + 3 H2O (1) --> 2 HNO3 (g) + NO (g)
Question 1 2 pts Which of the following reactions is likely to have a positive AS? 1. Nai) --> Na(s) II. 2 C4H10(g) + 13 O2(g) --> 8 CO2(g) + 10 H2O(g) III. CaCO3(s) + 2 HCl(aq) --> CaCl2(aq) + H200) + CO2(9) IV. 6 CO2(g) + 6 H20g) --> C6H12O6(s) +6 O2(g) I and IV II and III O II, III, and IV O I, II, III, and IV
Predict whether the entropy change for each of the following reactions will have a positive value or a negative value. Calculations are not necessary! (a) 2 CO (g) + 2 Cl2 (g) → 2 COCl2 (g) (b) 2 CO2 (g) → 2 CO (g) + O2 (g) (c) SiCl4 (g) + 2 H2O (g) → 4 HCl (g) + SiO2 (s, quartz)
Be sure to answer all parts. For each reaction, find the value of ΔSo. Report the value with the appropriate sign. (a) 3 NO2(g) + H2O(l) → 2 HNO3(l) + NO(g) 0.027 J/K (b) N2(g) + 3 F2(g) → 2 NF3(g) J/K (c) C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(g)
Which process is most likely to be spontaneous at standard temp and pressure? a. W(s) + 6CO(g) W(CO)6(s) b. H2O(g) H2O(l) c. C6H12O6(s) C6H12O6(aq) d. N2(g) + 3H2(g) 2NH
Select all of the following that you would predict to have a negative ΔS. a) 2 NO2 (g) → N2 (g) + 2 O2 (g) b) 2SO2 (g) + O2 (g) → 2 SO3 (g) c) 2 C6H6 (l) + 15 O2 (g) → 12 CO2 (g) + 6 H2O (g) d) 4 NO (g) + 6 H2O (g) → 4 NH3 (g) + 5 O2 (g) e) 2 BF3 (g) + 3 CaO (s) → B2O3 (s) + 3...
Select all options below that have a correct expression for the equilibrium constant. HOCI (aq) + HCl(aq) Cl2(aq) + H2O(1) K. = (CL2][H0] [HOCI](HCI) 2SC12(g) + O2(g) = 250Cl2(g) Po, · Pc SCl2 K, SOCL2 O2 NO2(aq) + H20 (1) - HNO2(aq) + HNO3(aq) (HNO2) + (HNO3] K (NO2)2 Camryn Butler: Attempt 1 лр Ploch O2 NO2(aq) + H20 (1) = HNO2(aq) + HNO3(aq) [HNO2] + [HNO3] (NO213 K. O HgO(s) Hg(0) + 1/2O2(g) Kc = [02]1/2 2Br2(g) + CH2(g)...
1) What is the ΔrG° for the following reaction (in kJ mol-1)? 2 Al (s) + Fe2O3 (s) ⇌ Al2O3 (s) + 2 Fe (s) 2) What is the ΔrG° for the following reaction (in kJ mol-1)? C6H12O6 (s, glucose) + 6 O2 (g) ⇌ 6 CO2 (g) + 6 H2O (l) 3) What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 2 Si (s) + 3 H2 (g) ⇌ Si2H6 (g) The conditions for...
1. Calculate the standard enthalpy of combustion for the following reaction: C6H12O6 (s) + 6 O2 (g) ---> 6 CO2 (g) + 6 H2O (l) To solve this problem, we must know the following ΔH°f values: C6H12O6 (s) -1275.0 O2 (g) zero CO2 (g) -393.5 H2O (l) -285.8 5. 2. Using the reaction and ΔH from #1, calculate how many liters of oxygen gas will be used to produce 11,000 kJ of energy at 745 mmHg and 90°C.
Which of the following is a typical chemical equation that represents a hydration reaction? 2 KClO3 (s) → 2 KCl (s) + 3 O2 (g) K2CO3 (s) ⟶H2O 2K+(aq) + CO3 2-(aq) HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l) C6H12O6 (s) + 6 O2 (g) → 6 CO2 (g) + 6 H2O (l)