For the reaction Cl2O(g) + 3/2O2(g) → 2ClO2(g) ΔH° = 126.4 kJ/mol and ΔS° = -74.9 J/K mol. At 381°C, what is ΔG?
it is a very simple problem of basic thermodynamics.All the symbols carry usual meaning .please rate and comment to improve myself.
For the reaction Cl2O(g) + 3/2O2(g) → 2ClO2(g) ΔH° = 126.4 kJ/mol and ΔS° = -74.9...
A certain reaction has ΔH°= -19.5 kJ/mol and ΔS°= +42.7 J/mol K a) Is the reaction exothermic or endothermic? b) Does the reaction lead to an increase or decrease in the disorder of the system? c) Calculate ΔG° for the reaction at 298K. d) Is the reaction spontaneous at 298 K under standard conditions?
For the following reaction: 2 CO(g) + O2(g) → 2 CO2(g), given ΔH = -566 kJ and ΔG = -514 kJ, find ΔS (J/K) at 25 oC. Multiple Choices: ΔS = -174 J/K ΔS = -0.174 J/K ΔS = -2.08J/K ΔS = 174 J/K ΔS = -2080 J/K
For a particular reaction, ΔH = -32 kJ and ΔS =-98 J/K. Assume that ΔH and ΔS do not vary withtemperature. A) At what temperature will the reaction have ΔG= 0? B) If T is increased from that in part A, will the reaction bespontaneous or nonspontaneous?
For a particular reaction at 205.1205.1 °C, ΔG=−45.90 kJ/molΔG=−45.90 kJ/mol, and ΔS=395.61 J/(mol⋅K)ΔS=395.61 J/(mol⋅K). Calculate ΔG for this reaction at −6.1−6.1 °C.
If the ΔH°rx and ΔS°rx for a gas phase chemical reaction are 419.53 kJ and -178.85 J/K respectively, determine ΔG°rx (in kJ) at 103.11 °C. Report your answer to two decimal places (i.e. 123.45 kJ). Assume that ΔH°rx and ΔS°rx do not vary with temperature.
Consider the Haber synthesis of gaseous NH3 (ΔH∘f = -46.1 kJ/mol; ΔG∘f = -16.5 kJ/mol): N2(g)+3H2(g)→2NH3(g) What are the equilibrium constants Kp and Kc for the reaction at 350 K ? You may assume that ΔH∘ and ΔS∘ are independent of temperature.
Consider the following reaction at 298 K. C(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/KC(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/K Calculate the following quantities. ΔSsys=ΔSsys J/K ΔSsurr= J/K ΔSuniv= J/K
Testbank, Question 033 Does a reaction with a ΔH of 20 kJ/mol and a ΔS of 10 J/mol·K at 298 K favor reactants or products?
Consider a reaction for which ΔH = 6.03 kJ/mol; ΔS = 22.1 J/K-mol. Which of the following statements is true? a. The reaction becomes spontaneous at high temperatures above 273 K b. The reaction becomes spontaneous at low temperatures below 273 K c. The reaction is spontaneous at all temperatures d. The reaction is never spontaneous
A reaction has ΔH∘rxn=−237 kJ and ΔS∘rxn= 218 J/K. Calculate ΔG∘rxn at 60 ∘C.