The equilibrium constant of a reaction at \[298\,K\] is \[5\times {{10}^{-3}}\] and at \[1000\,K\] is \[2\times {{10}^{-5}}\]. What is the sign of \[\Delta H\] for the reaction [Pb. CET 1998]

The equilibrium constant of a reaction at \[298\,K\] is \[5\times {{10

1.	The equilibrium constant of a reaction at \[298\,K\] is \[5\times {{10}^{-3}}\] and at \[1000\,K\] is \[2\times {{10}^{-5}}\]. What is the sign of \[\Delta H\] for the reaction [Pb. CET 1998]
A.	\[\Delta H=0\]
B.	\[\Delta H\] is negative
C.	\[\Delta H\] is positive
D.	None of these
Answer» C. \[\Delta H\] is positive

Discussion

No Comment Found

Related MCQs

In an isobaric process, the ratio of heat supplied to the system \[(dQ)\] and work done by the system \[(dW)\] for diatomic gas is [AFMC 2002]
To calculate the amount of work done in joules during reversible isothermal expansion of an ideal gas, the volume must be expressed in [KCET (Med.) 2001]
For the reaction \[{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\,\,\to \,\,{{H}_{2}}O(l),\,\Delta H=-285.8\,\,kJ\,\,mo{{l}^{-1}}\]\[\Delta S=-0.163\,kJ\,mo{{l}^{-1}}{{K}^{-1}}.\] What is the value of free energy change at \[{{27}^{o}}C\] for the reaction? [KCET 1999]
Following reaction occurring in an automobile \[2{{C}_{8}}{{H}_{18}}(g)+25{{O}_{2}}(g)\to 16C{{O}_{2}}(g)+18{{H}_{2}}O(g).\] The sign of \[\Delta H,\,\Delta S\] and \[\Delta G\] would be [CBSE PMT 1994; KCET 1999]
The heat content of a system is called
When \[50c{{m}^{3}}\] of \[0.2\,N\,{{H}_{2}}S{{O}_{4}}\] is mixed with \[50c{{m}^{3}}\] of \[1\,N\,KOH\], the heat liberated is [KCET 2004]
The \[{{H}_{2}}O(g)\] molecule dissociates as (i) \[{{H}_{2}}O(g)\to H(g)+OH(g);\,\Delta H=490\,kJ\] (ii) \[OH(g)\to H(g)+O(g);\,\Delta H=424\,kJ\] The average bond energy (in kJ) for water is
The equation \[\frac{1}{2}{{H}_{2}}+\frac{1}{2}C{{l}_{2}}\to HCl\] (\[\Delta {{H}_{298}}=-22060\,kcal\]) means [CMC Vellore 1991]
If at 298 K the bond energies of \[C-H,\,C-C,\] \[C=C\] and \[H-H\] bonds are respectively 414, 347, 615 and 435 kJ \[mo{{l}^{-1}}\], the value of enthalpy change for the reaction \[{{H}_{2}}C=C{{H}_{2}}(g)+{{H}_{2}}(g)\to {{H}_{3}}C-C{{H}_{3}}(g)\] at 298 K will be [AIEEE 2003]
Which of the following is not a correct statement? [AMU (Engg.) 2002]

The equilibrium constant of a reaction at \[298\,K\] is \[5\times {{10}^{-3}}\] and at \[1000\,K\] is \[2\times {{10}^{-5}}\]. What is the sign of \[\Delta H\] for the reaction [Pb. CET 1998]

Discussion

No Comment Found

Related MCQs

Reply to Comment