Multiple choice question
Multiple choice question Multiple choice question
4 0°C ij 3 eksy ty ds xyu ds fy;s ekud eqDr ÅtkZ ifjorZu (�G°) gS& (a) 'kwU; (b) (+)ve (c) (–)ve (d) buesa ls dksbZ ugh Standard free energy change (�G°) will be– (a) Zero (b) (+)ve (c) (–)ve (d) None of these 5 fxCl eqDr ÅtkZ (G), ,UFkSYih (H) rFkk ,UVªkWih (S) vkil esa lEcaf/kr gS& (a) G = H + TS (b) G = H – TS (c) G – TS = H (d) G = S = H Gibb’s free energy (G), enthalpy (H) and entropy (S) are related as– (a) G = H + TS (b) G = H – TS (c) G – TS = H (d) G = S = H 6 fdlh vkn'kZ xSl ds :)ks"e izlkj esa lnSo gksxk& (a) rkiØe es o`f) (b) �H = 0 (c) q = 0 (d) W = 0 For an ideal gas in its adiabatic expansion there is always– (a) Increase in Temperature (b) �H = 0 (c) q = 0 (d) W = 0 7 vxz ,oa mRØe vfHkfØ;k ds fy;s rFkk leku lfØ;.k ÅtkZ,sa j[kus okyh vfHkfØ;k ds fy;s& (a) �H = 0 (b) �S = 0 (c) 'kwU; dksfV (d) buesa ls dksbZ ugha For a forward and reversible reaction and for the reaction having same energies of activation. (a) �H = 0 (b) �S = 0 (c) Zero order (d) None of these 34
8 mRØe.kh; vfHkfØ;k ds fy;s lkE; voLFkk ij eqDr ÅtkZ ifjorZu gS& (a) 'kwU; ls vf/kd (b) 'kwU; ls de (c) 'kwU; ds cjkcj (d) buesa ls dksbZ ugha Free energy change for a reversible reaction at equilibrium is– (a) More than zero (b) Less than zero (c) Equal to zero (d) None of these 9 fdlh vkn'kZ xSl ds leryh; izlkj esa& (a) �E = 0 (b) W = 0 (c) dv = 0 (d) q = 0 For an ideal gas in an isothermal expansion– (a) �H = 0 (b) �S = 0 (c) Zero order (d) None of these 10 gSl dk fu;e vuqiz;ksx gS& (a) Å"ekxfrdh ds izFke fu;e dk (b) ,UVªkih ifjorZu (c) Å"ekxfrdh ds f}rh; fu;e dk (d) eqDr ÅtkZ ifjorZu dk Hess’s law is application of– (a) First law of thermodynamics (b) Entropy change (c) Second law of thermodynamics (d) Free energy change 11 fuEu esa ls fdlds fy;s �E = �H gksxk& (a) N 2 O 4(g) º 2NO 2(g) (c) H 2(g) + I 2(g) º 2HI (g) 35 (b) 2SO 2(g) + O 2(g) º 2SO 3(g) (d) H 2(g) + ½O 2(g) º H 2 O (l) Out of the above equations for which will be �E = �H (a) N 2 O 4(g) º 2NO 2(g) (c) H 2(g) + I 2(g) º 2HI (g) (b) 2SO 2(g) + O 2(g) º 2SO 3(g) (d) H 2(g) + ½O 2(g) º H 2 O (l)
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8 mRØe.kh; vfHkfØ;k ds fy;s lkE; voLFkk ij eqDr ÅtkZ ifjorZu gS&<br />
(a) 'kwU; ls vf/kd (b) 'kwU; ls de<br />
(c) 'kwU; ds cjkcj (d) buesa ls dksbZ ugha<br />
Free energy change for a reversible reaction at equilibrium is–<br />
(a) More than zero (b) Less than zero<br />
(c) Equal to zero (d) None of these<br />
9 fdlh vkn'kZ xSl ds leryh; izlkj esa&<br />
(a) �E = 0 (b) W = 0<br />
(c) dv = 0 (d) q = 0<br />
For an ideal gas in an isothermal expansion–<br />
(a) �H = 0 (b) �S = 0<br />
(c) Zero order (d) None of these<br />
10 gSl dk fu;e vuqiz;ksx gS&<br />
(a) Å"ekxfrdh ds izFke fu;e dk (b) ,UVªkih ifjorZu<br />
(c) Å"ekxfrdh ds f}rh; fu;e dk (d) eqDr ÅtkZ ifjorZu dk<br />
Hess’s law is application of–<br />
(a) First law of thermodynamics (b) Entropy change<br />
(c) Second law of thermodynamics (d) Free energy change<br />
11 fuEu esa ls fdlds fy;s �E = �H gksxk&<br />
(a) N 2 O 4(g) º 2NO 2(g)<br />
(c) H 2(g) + I 2(g) º 2HI (g)<br />
35<br />
(b) 2SO 2(g) + O 2(g) º 2SO 3(g)<br />
(d) H 2(g) + ½O 2(g) º H 2 O (l)<br />
Out of the above equations for which will be �E = �H<br />
(a) N 2 O 4(g) º 2NO 2(g)<br />
(c) H 2(g) + I 2(g) º 2HI (g)<br />
(b) 2SO 2(g) + O 2(g) º 2SO 3(g)<br />
(d) H 2(g) + ½O 2(g) º H 2 O (l)
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