The basic requirement for a process to be spontaneous depends on two parameters 1.Enthalpy
2.Entropy
So we will define spontaneity by the relation
∆G = ∆H - T ∆S
Delta GGmust be negative for reaction to be spontaneous
For a system to be spontaneous ∆S should be positive. If ∆S is positive, it means that the reaction can further take place till ∆S becomes 0 and so, the reaction is spontaneous. But if ∆S is negative, the reaction is non-spontaneous.
Gibbs free energy combines effect of both parameters and if Gibbs free energy comes out negative than process is spontaneous
As we have to make Delta G negative for Reaction will be spontaneous .
Case 1 Delta H = +ve Delta S = + ve
Reaction will be spontaneous at above a certain temperature
Case 2 ∆H= - ve. ∆ S= +ve
Reaction will be spontaneous at all temperature
Case 3 ∆H=-ve ∆S=-ve
Reaction will be spontaneous below certain range of temperature
Case 4 ∆H= +ve ∆S=-ve
Always non spontaneous so spontaneous in reverse direction
Classify the possible combinations of signs for a reaction's ΔΗ and AS values by the resulting...
Free Energy: Equilibrium Constant and Temperature Effects CHM1046 GEN CHEM WONLINE 619434 nergy: Equilibrium Constant and lemperature Effects Explain How Spontaneity is Affected by Temperature Question Consider the process below. How does the spontaneity of the process depend on temperature? 2SnO (s) 2SnO(s)+02(g) 584 kl mori, dS-220 J K-1 mol-1 ΔΗ Select the correct answer below O nonspontaneous at all temperatures spontaneous at all temperatures spontaneous above a certain temperature and nonspontaneous below spontaneous below a certain temperature and nonspontaneous...
em 11 Review Constants ! Predict the spontaneity of a reaction (and the temperature dependence of the spontaneity) for each possible combination of signs for AH and AS (for the system). Part A A negative, AS positive The reaction will be spontaneous at low temperature, but nonspontaneous at high temperature, The reaction will be nonspontaneous at all temperatures. The reaction will be spontaneous at all temperatures. The reaction will be nonspontaneous at low temperature, but spontaneous at high temperature. Submit...
How does the spontaneity of the process below depend on temperature? PCI5(9)+H2O(g)POCI3(g) +2HCI(g) -126 kJ mol1, AS = 146 J K-'mol1 ΔΗ Select the correct answer below: nonspontaneous at all temperatures spontaneous at all temperatures spontaneous at high temperatures and nonspontaneous at low temperatures spontaneous at low temperatures and nonspontaneous at high temperatures
Which of the following describes the temperature dependence of the spontaneity of the reaction below? 2H202(0) 2H2O()+02(g) ΔΗ--196kl mol-1, AS-126 J K-1 mol-i Select the correct answer below: 0 O O O nonspontaneous at all temperatures spontaneous at all temperatures spontaneous at high temperatures and nonspontaneous at low temperatures spontaneous at low temperatures and nonspontaneous at high temperatures
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) CaH, (s) + 2 H20 (1) - Ca(OH)2 (s) + 2 H, (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) 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 (1); (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 (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...
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) PbS (s) + Mg (s) → Mg (s) + Pb (s); ∆H = 66 kJ; ∆S = -9 J/K (b) 2 SO2 (g) + O2 (g) → 2 SO3 (g);...