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Thermal decomposition of gaseous X_(2) to gaseousX at 298 K takes place according to the equation : X_(2) (g) hArr 2X (g) The standard reaction Gibbs energy , Delta_(r)G^(@) of this reaction is positive . At the start of the reaction, there is positive . At the start of the reaction , there is one mole of X_(2) andno. As the reaction proceeds, the number of moles of X formed is given by beta." Thus " beta _(equilbrium )is the number ofmoles of X formed at equilibrium . The reaction is carried out at a constant total pressure of 2 bar . Consider the gases to behave ideally . ( Given : R = 0* 0833 " L bar " K^(-1)mol^(-1)). The INCORRECT statement among the following for this reaction is |
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Answer» Decrease in the total pressure will result in formation of more moles of gaseous X (b) At the start of the reaction , `Q LT V` Hence, reaction will proceed in the forward direction . So (b) is also correct. (c) If `beta_(eq.) = 0*7 , " then " K = (8 xx (0*7)^(2))/(4 - (0*7)^(2) ) gt 1 ` `Delta G^(@) =-RT "In" K_(p) :.Delta G^(@) "will be" - "ve but we are given that " Delta G^(@)" is " +" ve which can be so if " K_(p) lt 1. " Hence " beta_(eq.) !=0*7 , " i.e, (c) is incorrect . "` (d) `K_(p) = K_(c) (RT)^(Deltan_(g))= K_(c) (RT) or K_(c) = K_(p)/(RT)`. Thus, `K_(c) lt K_(p)` As `K_(p) lt 1, "therefore " K_(c) lt 1. ` Hence, (d) is also correct. |
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