For the reaction below, which statement best describes what is happening with thesign of AGO?CrP O46)+3 N a Cla q) - N agP O4la q) * CrClata qllendothermic)The reaction is spontaneous at low temperature and non-spontaneous at hightemperature.The reaction is non-spontaneous at all temperatures.The reaction is non-spontaneous at low temperature and spontaneous at hightemperature.The reaction is spontaneous at all temperatures.

The chemical equation may be written as: CrPO4(s) + 3NaCl(aq)→ CrCl3(aq) + Na3PO4(aq) Number of ions…

Answered: For the reaction below, which statement…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

For the reaction below, which statement best describes what is happening with the
sign of AGO?
CrP O46)+3 N a Cla q) - N agP O4la q) * CrClata qllendothermic)
The reaction is spontaneous at low temperature and non-spontaneous at high
temperature.
The reaction is non-spontaneous at all temperatures.
The reaction is non-spontaneous at low temperature and spontaneous at high
temperature.
The reaction is spontaneous at all temperatures.

Expert Solution

Step 1

The chemical equation may be written as:

$C r P O_{4} (s) + 3 N a C l (a q) \to C r C l_{3} (a q) + N a_{3} P O_{4} (a q)$

$N u m b e r o f i o n s a n d m o l e c u l e s o n l e f t h a n d s i d e = o n e s o l i d e q u a l t o 1 a n d 3 m o l e o f N a C l e q u a l t o 6 m o l e o f i o n s t o t a l = 7 m o l e$

On the right side (products) one mole of

CrCl₃→ Cr⁺³ + 3Cl^- ( 4 mole ions)

and

Na₃PO₄→ 3Na⁺ + PO₄^-3 ions (4 mole ions) total moles on right side 8 moles

So, in this reaction number of moles from left to right increase hence ΔS⁰ is +ve and it is an endothermic reaction ΔH⁰ is +ve

Step 2

Free energy decides spontaneity of a reaction

Mathematically,

Apply in Gibbs equation

$Δ G ° = Δ H ° - T Δ S °$

Where,

$∆$ G $°$ = Gibb's free energy

$∆$ H $°$ = Change in enthalpy

T = Temperaature

$∆$ S $°$ = Change in entropy

Since, ΔH $°$ is +ve and ΔS $°$ is +ve then ΔG $°$ become -ve at high temperatures.

Step 3

Criteria for the spontaneity:

(i)

If $∆$ G = 0, reaction is in equilibrium.

(ii) If $∆$ G = -ive i.e $∆$ G<0, reaction is spontaneous.

(iii) If $∆$ G = +ive i.e $∆$ G>0, reaction is non-spontaneous.

For endothemic reaction change in entropy always positive,

$∆$ H = + ive value.

For exothermic

$∆$ H = - ive value.

Entropy of any irreversible reaction is positive.

Step 4

$Δ G ° = Δ H ° - T Δ S °$

since this is endothermic reaction

$∆$ H = + ive value.

so, if temperature is low,

$∆$ H >T $∆$ S

$∆$ G is +ive( non- spontaneous)

At high temperature

$∆$ H <T $∆$ S

Therefore, $∆$ G is -ive( spontaneous)

At lower temperature it will non spontaneous.

Hence, option A is inncorrect.

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