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16. For the following reactions, predict whether they will tend to be spontaneous at either high...
15. The standard Gibbs free energy change (AG%) for the Haber reaction at 298K is -2.83...
15. The standard Gibbs free energy change (AG%) for the Haber reaction at 298K is -2.83 kJ/mol N2(g) + 3H2(g) + 2NH3(g) If the reaction begins with 2.55 atm N2(g) 0.115 atm Hz(g) and 0.488 atm NH3(9) at 298K what is the free energy change (AG) for the reaction under these conditions AND will the reaction be spontaneous under these conditions? (10 points) 16. For the following reactions, predict whether they will tend to be spontaneous at either high or...
14. For the following reactions, predict whether they will tend to be spontaneous at high, low,...
14. For the following reactions, predict whether they will tend to be spontaneous at high, low, all temperatures, or non-spontaneous at any temperature (10 points) a) An "instant ice-pack" type of reaction where AS > 0, and AH > 0 b) 3A (1) ► B(s) + C(1) + D(g), AH < 0 c) 2A(s) → B(g) + C(1), AH > 0
please answer 9a,b,c,d 9. For the following reactions, predict whether they will tend to be spontaneous...
please answer 9a,b,c,d
9. For the following reactions, predict whether they will tend to be spontaneous at high, low, ali temperatures, or non-spontaneous at any temperature (10 points) a) 2A(g) + 3B(9) C(g) + D(1), AH < 0 b) A() + B() (1) + D(s) AH > 0 c) A(s) + B(1) ► 20(1), AH < 0 d) 2A(s) B(s) + C(I), AH > 0
State whether following reactions are spontaneous at all temperatures, low temperatures, high temperatures or not spontaneous...
State whether following reactions are spontaneous at all temperatures, low temperatures, high temperatures or not spontaneous at any temperatures. (a) N2(g) + 3 F2(g) + 2 NF3(g) AH = -249 kJ (b) N()+ 3Cl2(g) → 2 NC13(g) AH = 460 kJ (e) NF4(8) 2 NF2(g) AH = 85 kJ
4. Classify each of the following reactions as one of these four types: • spontaneous at...
4. Classify each of the following reactions as one of these four types: • spontaneous at all temperatures • not spontaneous at any temperature • spontaneous below a certain temperature but not above • spontaneous above a certain temperature but not below See Table 17.1 in Tro, Fridgen and Shaw. (a) CaH2 () + 2 H2O (1) + Ca(OH)2 (s) + 2 H2(g); AH = -230 kJ; (b) 2 NO(g) + Cl, (g) → 2 NOCI (g); AH= -78.4 kJ;...
4. Classify each of the following reactions as one of these four types: • spontaneous at...
4. Classify each of the following reactions as one of these four types: • spontaneous at all temperatures • not spontaneous at any temperature • spontaneous below a certain temperature but not above • spontaneous above a certain temperature but not below See Table 17.1 in Tro, Fridgen and Shaw. (a) 2 SO, (g) → 2 SO, (g) + O2(g); (b) Be(OH). (s) + H2(g) → Be (s) + 2 H2O (L); (c) CH. (g) + H2(g) → CH(g); (d)...
4. Classify each of the following reactions as one of these four types: • spontaneous at...
4. Classify each of the following reactions as one of these four types: • spontaneous at all temperatures • not spontaneous at any temperature • spontaneous below a certain temperature but not above • spontaneous above a certain temperature but not below See Table 17.1 in Tro, Fridgen and Shaw. (a) 2 SO, (g) 2 SO, (g) + O2(g); (b) Be(OH), (s) + H2(g) → Be (s) + 2 H2O (1); (c) CH. (g) + H2(g) → CH. (g); (d)...
Predict whether AS will be positive or negative for reactions (a) and (b): a. 2 HgO(s)...
Predict whether AS will be positive or negative for reactions (a) and (b): a. 2 HgO(s) → 2Hg(1) + O2(g) AS b. 2 CH (B) + 70(8) ► 4 CO2(g) + 6 H2O(1) AS Choose one of the above reactions a OR b. Calculate the AH® for your chosen reaction using information from the table below. AH = Using your answers above, predict under what temperature (temp) conditions (high temp or low temp) where this reaction will be spontaneous, or...
4. Classify each of the following reactions as one of these four types: • spontaneous at...
4. Classify each of the following reactions as one of these four types: • spontaneous at all temperatures • not spontaneous at any temperature • spontaneous below a certain temperature but not above • spontaneous above a certain temperature but not below (a) CO (g) + 3 H2 (g) → CH4 (g) + H2O (g); ∆H = -206.1 kJ; ∆S = -214.6 J/K (b) AgClO3 (s) + CH4 (g) → AgCl (s) + 2 H2O (g) + CO (g); ∆H...
4. Classify each of the following reactions as one of these four types: • spontaneous at...
4. Classify each of the following reactions as one of these four types: • spontaneous at all temperatures • not spontaneous at any temperature spontaneous below a certain temperature but not above • spontaneous above a certain temperature but not below See Table 17.1 in Tro, Fridgen and Shaw. AS = -198.8 J/K AH = 924 kJ; AS = (a) N2(g) + 3 H2(g) → 2 NH, (g); AH = -92.2 kJ; (b) 2 Na O (s) + 5 CO2(g)...
15. The standard Gibbs free energy change (AG%) for the Haber reaction at 298K is -2.83 kJ/mol N2(g) + 3H2(g) + 2NH3(g) If the reaction begins with 2.55 atm N2(g) 0.115 atm Hz(g) and 0.488 atm NH3(9) at 298K what is the free energy change (AG) for the reaction under these conditions AND will the reaction be spontaneous under these conditions? (10 points) 16. For the following reactions, predict whether they will tend to be spontaneous at either high or...
14. For the following reactions, predict whether they will tend to be spontaneous at high, low, all temperatures, or non-spontaneous at any temperature (10 points) a) An "instant ice-pack" type of reaction where AS > 0, and AH > 0 b) 3A (1) ► B(s) + C(1) + D(g), AH < 0 c) 2A(s) → B(g) + C(1), AH > 0
please answer 9a,b,c,d
9. For the following reactions, predict whether they will tend to be spontaneous at high, low, ali temperatures, or non-spontaneous at any temperature (10 points) a) 2A(g) + 3B(9) C(g) + D(1), AH < 0 b) A() + B() (1) + D(s) AH > 0 c) A(s) + B(1) ► 20(1), AH < 0 d) 2A(s) B(s) + C(I), AH > 0
State whether following reactions are spontaneous at all temperatures, low temperatures, high temperatures or not spontaneous at any temperatures. (a) N2(g) + 3 F2(g) + 2 NF3(g) AH = -249 kJ (b) N()+ 3Cl2(g) → 2 NC13(g) AH = 460 kJ (e) NF4(8) 2 NF2(g) AH = 85 kJ
4. Classify each of the following reactions as one of these four types: • spontaneous at all temperatures • not spontaneous at any temperature • spontaneous below a certain temperature but not above • spontaneous above a certain temperature but not below See Table 17.1 in Tro, Fridgen and Shaw. (a) CaH2 () + 2 H2O (1) + Ca(OH)2 (s) + 2 H2(g); AH = -230 kJ; (b) 2 NO(g) + Cl, (g) → 2 NOCI (g); AH= -78.4 kJ;...
4. Classify each of the following reactions as one of these four types: • spontaneous at all temperatures • not spontaneous at any temperature • spontaneous below a certain temperature but not above • spontaneous above a certain temperature but not below See Table 17.1 in Tro, Fridgen and Shaw. (a) 2 SO, (g) → 2 SO, (g) + O2(g); (b) Be(OH). (s) + H2(g) → Be (s) + 2 H2O (L); (c) CH. (g) + H2(g) → CH(g); (d)...
4. Classify each of the following reactions as one of these four types: • spontaneous at all temperatures • not spontaneous at any temperature • spontaneous below a certain temperature but not above • spontaneous above a certain temperature but not below See Table 17.1 in Tro, Fridgen and Shaw. (a) 2 SO, (g) 2 SO, (g) + O2(g); (b) Be(OH), (s) + H2(g) → Be (s) + 2 H2O (1); (c) CH. (g) + H2(g) → CH. (g); (d)...
Predict whether AS will be positive or negative for reactions (a) and (b): a. 2 HgO(s) → 2Hg(1) + O2(g) AS b. 2 CH (B) + 70(8) ► 4 CO2(g) + 6 H2O(1) AS Choose one of the above reactions a OR b. Calculate the AH® for your chosen reaction using information from the table below. AH = Using your answers above, predict under what temperature (temp) conditions (high temp or low temp) where this reaction will be spontaneous, or...
4. Classify each of the following reactions as one of these four types: • spontaneous at all temperatures • not spontaneous at any temperature spontaneous below a certain temperature but not above • spontaneous above a certain temperature but not below See Table 17.1 in Tro, Fridgen and Shaw. AS = -198.8 J/K AH = 924 kJ; AS = (a) N2(g) + 3 H2(g) → 2 NH, (g); AH = -92.2 kJ; (b) 2 Na O (s) + 5 CO2(g)...
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