Question

In: Chemistry

Consider a reaction with the following thermodynamic properties. ΔH° = 77.7 kJ ΔS° = –35.7 J/(K...

Consider a reaction with the following thermodynamic properties.

ΔH° = 77.7 kJ
ΔS° = –35.7 J/(K • mol)
ΔG°= 88.4 kJ

This reaction:

will proceed very slowly.

will be spontaneous at low temperatures.

has bonds in the products that are weaker than the reactants.

may have fewer and more complicated molecules in the product.

Solutions

Expert Solution

* This reaction will proceed very slowly.

* This reaction has bonds in products that are weaker than the reactants.

* This reaction may have fewer and more complicated molecules in the product.


Related Solutions

Use the values found in Thermodynamic Properties to determine ΔS°, ΔH° and ΔG° at 298 K...
Use the values found in Thermodynamic Properties to determine ΔS°, ΔH° and ΔG° at 298 K for the reaction below. Enter all values to the 0.1 place. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) ΔS° ΔH° ΔG°
Part A ΔH∘rxn=− 93 kJ , ΔS∘rxn=− 147 J/K , T= 304 K Express your answer...
Part A ΔH∘rxn=− 93 kJ , ΔS∘rxn=− 147 J/K , T= 304 K Express your answer using two significant figures. ΔG Δ G = kJ Previous AnswersRequest Answer Incorrect; Try Again; 5 attempts remaining Part B ΔH∘rxn=− 93 kJ , ΔS∘rxn=− 147 J/K , T= 858 K Express your answer using two significant figures. ΔG Δ G = nothing kJ Request Answer Part C ΔH∘rxn= 93 kJ , ΔS∘rxn=− 147 J/K , T= 304 K Express your answer using two...
S(s,rhombic) + 2CO(g) ------> SO2(g) + 2C(s,graphite) ΔH° = -75.8 kJ and ΔS° = -167.6 J/K...
S(s,rhombic) + 2CO(g) ------> SO2(g) + 2C(s,graphite) ΔH° = -75.8 kJ and ΔS° = -167.6 J/K The maximum amount of work that could be done when 1.81 moles of S(s,rhombic) react at 323 K, 1 atm is _______ kJ. Assume that ΔH° and ΔS° are independent of temperature. Please answer it kJ
A) It is determined that for a particular process, ΔH = +185 kJ and ΔS =...
A) It is determined that for a particular process, ΔH = +185 kJ and ΔS = +1.80 J/K. At what temperature (in kelvin) does the reaction become spontaneous? B)Which of the following statements are true for the reaction I2(g) → 2 I(g) I. ΔH is positive II. ΔH is negative III. ΔS is positive IV. ΔS is negative V. The reaction is spontaneous at any temperature C) For which of the following processes would ΔS° be expected to be most...
Given the values of ΔH∘rxn, ΔS∘rxn, and Tbelow, determine ΔSuniv. A. ΔH∘rxn=− 118 kJ , ΔS∘rxn=...
Given the values of ΔH∘rxn, ΔS∘rxn, and Tbelow, determine ΔSuniv. A. ΔH∘rxn=− 118 kJ , ΔS∘rxn= 258 J/K , T= 294 K B. ΔH∘rxn= 118 kJ , ΔS∘rxn=− 258 J/K , T= 294 K C. ΔH∘rxn=− 118 kJ , ΔS∘rxn=− 258 J/K , T= 294 K . D. ΔH∘rxn=− 118 kJ , ΔS∘rxn=− 258 J/K , T= 545 K . Predict whether or not the reaction in part A will be spontaneous. Predict whether or not the reaction in part...
For a particular reaction at 129.9 °C, ΔG = 319.61 kJ/mol, and ΔS = 777.00 J/(mol·K)....
For a particular reaction at 129.9 °C, ΔG = 319.61 kJ/mol, and ΔS = 777.00 J/(mol·K). delta g is -47.6 celcius
For a particular reaction at 234.1 °C, ΔG = -832.94 kJ/mol, and ΔS = 923.32 J/(mol·K)....
For a particular reaction at 234.1 °C, ΔG = -832.94 kJ/mol, and ΔS = 923.32 J/(mol·K). Calculate ΔG for this reaction at -105.7 °C.
For a particular reaction at 215.7 °C, ΔG = 404.91 kJ/mol, and ΔS = 748.20 J/(mol·K)....
For a particular reaction at 215.7 °C, ΔG = 404.91 kJ/mol, and ΔS = 748.20 J/(mol·K). Calculate delta G for -74.3 celcius. I've asked this question previously and the individual who answered got roughly 378 kj/mol which is incorrect.
Consider the following reaction: PCl5 (g)⇄ PCl3 (g) + Cl2 (g) ΔH = 87.9 kJ/reaction For...
Consider the following reaction: PCl5 (g)⇄ PCl3 (g) + Cl2 (g) ΔH = 87.9 kJ/reaction For each of the following changes, indicate whether the reaction will proceed towards products, towards reactants, or have no net reaction to reestablish equilibrium. a. ___________ Temperature is increased b. ___________ The pressure is increased by decreasing the volume. c. ___________ The pressure is decreased by removing some PCl 5 (g) d. ___________ The pressure is increased by adding N2(g) e. ___________ Cl2(g) is removed...
For a particular reaction at 129.9 °C, ΔG = -603.84 kJ/mol, and ΔS = 313.84 J/(mol·K).Calculate...
For a particular reaction at 129.9 °C, ΔG = -603.84 kJ/mol, and ΔS = 313.84 J/(mol·K).Calculate ΔG for this reaction at -3.4 °C.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT