A mixture of hydrogen and chlorine remains unreacted until it is exposed to ultr

Question

A mixture of hydrogen and chlorine remains unreacted until it is exposed to ultraviolet light from burning magnesium strip. Then the following reaction occurs very rapidly: H_2(g) + Cl_2(g) 2HCl(g) Delta G =-45.54 kJ Delta H =-44.12 kJ Delta S = -4.76 J/K Which of the following is consistent with this information? The reaction has a small equilibrium constant. The ultraviolet light raises the temperature of the system and makes the reaction more favorable. The negative value for AS slows down the reaction. The reaction is spontaneous, but the reactants are kinetically stable.

Explanation / Answer

A)
delta G = -R*T*ln K
Value of delta G is highly negative. SO K will be large
So A is wrong

B)
delta G = delta H - T* delta S
since delta S is negative, raising the temprature will make delta G less negative and reaction will become less favourable
So B iswrong

C)
delta S is thermodynamic property.It has no effect on Kinetics of reaction
Hence this is False

D)
It is true
delta G is negative. So reaction is spontaneous
Also H2 and Cl2 are stable

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.