A) If ΔH = -70.0 kJ and ΔS = -0.400 kJ/K , the reaction is spontaneous...
A) If ΔH = -70.0 kJ and ΔS = -0.400 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature.
Express your answer numerically in kelvins.
B) Glacial acetic acid is the concentrated form of acetic acid, the acid in vinegar. The term "glacial" refers to the appearance of the solid form, which resembles ice-like crystals. What is the melting point of this compound, in degrees Celsius, based on its thermodynamic data shown here?
| ΔHfus (kJ/mol) |
ΔSfus [J/(K⋅mol)] |
| 24.32 | 83.93 |
Express the melting point numerically in degrees Celsius.
C) The standard Gibbs free energy of formation of ________ is
zero.
(a) H2O(l)
(b) O(g)
(c) Br2(l)
| (a) only |
| (b) only |
| (c) only |
| (b) and (c) |
| (a), (b), and (c) |
D) The value of ΔG∘ at 120.0∘C for the formation of phosphorous
trichloride from its constituent elements,
P2(g)+3Cl2(g)→2PCl3(g)
is ________ kJ/mol. At 25.0∘C for this reaction, ΔH∘ is
−720.5kJ/mol, ΔG∘ is −642.9kJ/mol, and ΔS∘ is −263.7J/K.
| 3.09×10^4 |
| −616.8 |
| −824.2 |
| 1.03×10^5 |
| −688.9 |
Homework Answers
Add Answer to:
A) If ΔH = -70.0 kJ and ΔS = -0.400 kJ/K , the reaction is
spontaneous...
At equilibrium, the free energy change, ΔG, of any system is zero: ΔG=0=ΔH−TΔS So, under equilibrium...
At equilibrium, the free energy change, ΔG, of any system is zero: ΔG=0=ΔH−TΔS So, under equilibrium conditions, this equation can be rearranged as T=ΔHΔS Part A Glacial acetic acid is the concentrated form of acetic acid, the acid in vinegar. The term "glacial" refers to the appearance of the solid form, which resembles glacial ice. What is the melting point of this compound, in degrees Celsius, based on its thermodynamic data shown here? ΔHfus (kJ/mol) = 24.32 ΔSfus [J/(K⋅mol)] =...
Part A Part complete Glacial acetic acid is the concentrated form of acetic acid, the acid...
Part A Part complete Glacial acetic acid is the concentrated form of acetic acid, the acid in vinegar. The term "glacial" refers to the appearance of the solid form, which resembles glacial ice. What is the melting point of this compound, in degrees Celsius, based on its thermodynamic data shown here? ΔHfus (kJ/mol) ΔSfus [J/(K⋅mol)] 24.32 83.93 Express the melting point numerically in degrees Celsius. View Available Hint(s) 16.6 ∘C SubmitPrevious Answers Correct Part B Based on the following thermodynamic...
The value of ΔG° at 241.0°C for the formation of phosphorous trichloride from its constituent elements,...
The value of ΔG° at 241.0°C for the formation of phosphorous trichloride from its constituent elements, P2(g) + 3Cl2(g) → 2PCl3(g) is ________ kJ/mol. At 25.0°C for this reaction, ΔH° is -720.5 kJ/mol, ΔG° is -642.9 kJ/mol, and ΔS° is -263.7 J/K.
If ΔH = -70.0 kJ and ΔS = -0.300 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temper...
If ΔH = -70.0 kJ and ΔS = -0.300 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature. Express your answer numerically in kelvins.
The value of ΔG∘ at 221.0∘C for the formation of phosphorous trichloride from its constituent elements,...
The value of ΔG∘ at 221.0∘C for the formation of phosphorous trichloride from its constituent elements, P2(g)+3Cl2(g)→2PCl3(g) is ________ kJ/mol. At 25.0∘C for this reaction, ΔH∘ is −720.5kJ/mol, ΔG∘ is −642.9kJ/mol, and ΔS∘ is −263.7J/K. −662.2 −590.2 1.30×105 −850.8 5.76 ×104
1. Consider a process at 286 K with ΔH = -72.5 kJ/mol and ΔS = -96.8...
1. Consider a process at 286 K with ΔH = -72.5 kJ/mol and ΔS = -96.8 J/K mol Which of the following is true? ΔG = -44.8 kJ/mol and the process will not be spontaneous ΔG = +39.4 kJ/mol and the process will be spontaneous ΔG = -44.8 kJ/mol and the process will be spontaneous ΔG = -19.1 kJ/mol and the process will not be spontaneous ΔG = +39.4 kJ/mol and the process will not be spontaneous 2. Consider a...
Consider a process at 286 K with ΔH = -72.5 kJ/mol and ΔS = -96.8 J/K...
Consider a process at 286 K with ΔH = -72.5 kJ/mol and ΔS = -96.8 J/K mol Which of the following is true? ΔG = -19.1 kJ/mol and the process will not be spontaneous ΔG = -44.8 kJ/mol and the process will not be spontaneous ΔG = -44.8 kJ/mol and the process will be spontaneous ΔG = +39.4 kJ/mol and the process will not be spontaneous ΔG = +39.4 kJ/mol and the process will be spontaneous
Part C If ΔH = -80.0 kJ and ΔS = -0.200 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that...
Part C If ΔH = -80.0 kJ and ΔS = -0.200 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature. Express your answer numerically in kelvins.
1. If If Kc=0.425 at 40.°C and Kc=0.670 at 90.°C, what is ΔH° for the reaction?...
1. If If Kc=0.425 at 40.°C and Kc=0.670 at 90.°C, what is ΔH° for the reaction? X↽−−⇀Y kj 2.Consider a general reaction A(aq)⇌enzymeB(aq) The ΔG°′ of the reaction is −7.500 kJ·mol−1. Calculate the equilibrium constant for the reaction at 25 °C. Keq′= What is ΔG for the reaction at body temperature (37.0 °C) if the concentration of A is 1.7 M and the concentration of B is 0.65 M? ΔG= 3. Attempt 9 Consider the data in the table. Compound...
If ΔH = -80.0 kJ and ΔS = -0.500 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temper...
If ΔH = -80.0 kJ and ΔS = -0.500 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature Express your answer numerically in kelvins.
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