An example of a nonspontaneous process with negative ∆H0 and negative ∆S0 would be
a. |
H2O(g) -> H2O(l) at 1050C
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b. |
H2O(g) -> H2O(l) at 950C |
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d. |
H2O(l) -> H2O(g) at 1050C |
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e. |
H2O(l) -> H2O(g) at 950C |
An example of a nonspontaneous process with negative ∆H0 and negative ∆S0 would be a. H2O(g)...
For the following example, identify the following. H2O(l) + H2O(g) a negative AH and a positive AS a positive AH and a positive AS It is not possible to determine without more information. a positive AH and a negative AS O a negative AH and a negative AS
1. For the process H2O(g) → H2O(l) at 105°C the signs on AG, AH, and AS are a)-, t, + b)t, -, - c) +, +, + d) +, t, - e)-, -, - 2. For the process H2O(l) → H2O(s) at -5°C the signs on AG, AH, and AS are a)-, +, + b) +, -, - c) +, +, + d) +, +, - e)-,-,- 3. For the process H2O(s) → H2O(l) at +5°C the signs on AG,...
IF ÄH and ÄS are both negative for a reaction, then the reaction is: a. nonspontaneous at low temperatures and spontaneous at high temperatures. b. spontaneous at low temperatures and nonspontaneous at high temperatures. C. spontaneous at all temperatures. d. nonspontaneous at all temperatures. e. none of the choices given above Suppose that AH° = +95.1 kJ and AS° =-0.192 kJ/K for a chemical reaction. What is AG at 600 K? a. +20.1 kJ b.-20.1 kJ c. +152.3k) d.+210.3 kJ...
(a) We define standard Gibbs energy change, G0 = H0 – TS0, what is the relationship between G0 and Suniv you have calculated in previous problem? (b ) Take H0 , S0 values you got in problem 2; get G0 value at T=298K,what is the sign of G0? What does that tell you about the process being spontaneous or not? (c ) Find the temperature at which G0 =0(you may assume H0 and S0 donot change with temperature). What is...
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
At 25 °C, the following reaction is CH4(9) + 2O2(g) + CO2(g) + 2 H2O(1) Nonspontaneous due to unfavorable enthalpy Spontaneous with favorable enthalpy and entropy Spontaneous with favorable enthalpy change Spontaneous with favorable entropy change
2. For the following example, identify the following. H2O(l) → H2O(s) question 2 options a negative ΔH and a negative ΔS a positive ΔH and a negative ΔS a negative ΔH and a positive ΔS a positive ΔH and a positive ΔS It is not possible to determine without more information. 3. Calculate ΔS°rxn for the following reaction. The S° for each species is shown below the reaction. C2H2(g) + H2(g) → C2H4(g) S°(J/mol∙K) 200.9 130.7 219.3 Question 4 options:...
which process is associated with a negative entropy change? why? A) NaCl(s) -> Na+(aq) + Cl-(aq) B) N2(g) + 3H2(g) -> 2NH3(g) C) 2BrCl(l) -> Br2(l) + Cl2(g) D) H2O (l) -> H2O (g)
Which of the following processes has a negative AS? A) CaCO3(s) → Cao(s) + CO2(g) B) H2O(g) → H2O(s) C) CO2(s) + CO2(g) D) C6H1206(s) → C6H1206(aq) E) AS cannot be negative
An example of a reaction where ∆G = 0 is H2O(s)→H2O(l) @SATP any reaction that is over H2O(g)→H2O(l) @SATP all combustion reactions