Question 7According to the table below, which statement describes an exothermic reaction in whichthe randomness decreases?Enthalpy Change Entropy Change Spontaneous Reaction?Exothermic (-AH)Increase (+AS) | Yes, -AG at any temperatureExothermic (-AH)Decrease (-AS) | Only at low temps, if |T AS| < JAH|Endothermic (+AH)Increase (+AS) | Only at high temps, if |T AS| > JAH|Endothermic (+AH) | Decrease (-AS) No, +AG at any temperatureAIt is spontaneous at all temperatures.It is not spontaneous at any temperature.It is spontaneous only at lower temperatures.It is spontaneous only at higher temperatures.

Spontaneous reaction can be defined as the reaction that occur by itself without any external source…

Question 7 According to the table below, which statement desc the randomness decreases? Enthalpy Change Entropy Change Sp Exothermic (-AH) Increase (+AS) Yes Exothermic (-AH) Decrease (-AS) On Endothermic (+AH) | Increase (+AS) On Endothermic (+AH) Decrease (-AS) No A It is spontaneous at all temperatures. It is not spontaneous at any temperature. It is spontaneous only at lower temperatures. It is spontaneous only at higher temperatures.

Question 7 According to the table below, which statement desc the randomness decreases? Enthalpy Change Entropy Change Sp Exothermic (-AH) Increase (+AS) Yes Exothermic (-AH) Decrease (-AS) On Endothermic (+AH) | Increase (+AS) On Endothermic (+AH) Decrease (-AS) No A It is spontaneous at all temperatures. It is not spontaneous at any temperature. It is spontaneous only at lower temperatures. It is spontaneous only at higher temperatures.

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter4: Polar Bonds, Polar Reactions

Section: Chapter Questions

Problem 29CTQ

See similar textbooks

Similar questions

a)Determine ∆Grxno values for the following combustion reactions at 25oC b) Decide whether this reaction is spontanious at 25oC or not CH4(g)+O2(g)→CO2(g)+H2O(I) ∆Hf°(kj/mol) S°(KJ/mol) CH4 -74.87 0.186 O2 0 0.205 CO2 -393.51 0.214 H2O -285.83 0.070
Activity 2-13 1. Derive the expression for getting the entropy changes in a chemical reaction. And why is the third law useful?
Suppose you have an endothermic reaction with H = + 15 kJ and a S of 150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
Suppose you have an exothermic reaction with H = 15 kJ and a S of +150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
What is a nonspontaneous reaction?
At 25oC, Ksp for copper(I) chloride (CuCl) is 1.0 x 10-6. Calculate ΔΔGo (kJ/mol) for the reaction: CuCl(s) ⇆ Cu+(aq) + Cl-(aq) Select one: a. 34.2 kJ/mol b. 3.42 x 104 kJ/mol c. -3.42 x 104 kJ/mol d. -34.2 kJ/mol
I this calculation of the enthalpy of a reaction as measured in a constant pressure telemetry container, I totally get everything except for the exothermic part. I understand that hcl at 25 C mixed with NaOH at 25 degrees gives off h20 and heat, thus exothermic. But what puzzles me is why the formula q = s m delta T yields a positive number indicating an endothermic process. ( final temp higher than initial)
Calculatre the ΔH of reaction for the following reaction: Fe3O4 (s) + CO (g) --> 3FeO (s) + CO2 (g) ΔHfo (kJ/mol) -1118 -110.5 -272 -393.5 a -263 kJ b 54 kJ c 19 kJ d -50 kJ e 109 kJ
At 400 C, Kc is 8.05 x 10 -4 for the reaction COCl2(g) -- CO(g) + Cl2(g) Calculate Go from this value of Kc
DG° < 0, DH° < 0 and DS° < 0 is it this if the reaction is H2O (l) →→ H2O (s) occurring at -20°C and standard conditions..
What is the balanced net inotic equation for: Pb+2(aq)+SO4-2 ----> ?
At 25oC, for the reaction 2 A(aq) ----> B(aq) + C(aq), the equilibrium constant is 1.79 . If the concentration of B(aq) were 0.311 M and the concentration of C(aq) were 0.477 M, what would be the minimum concentration of A(aq) required (in mol/L) to make this reaction spontaneous under these conditions?