Calculate Delta S degree for the reaction SiCl_4(g) + 2Mg(s) rightarrow 2MgCl_2(

Question

Calculate Delta S degree for the reaction SiCl_4(g) + 2Mg(s) rightarrow 2MgCl_2(s) + Si(s) A) -254.96 J/K B) -198.02 J/K C) 198.02 J/K D) 254.96 J/K E) 471.86 J/K Calculate the entropy change for vaporization of 18 g of H_2O. The molar enthalpy of vaporization for water is 44 kJ/mol and the boiling point is 100 degree C. A) 44 kJ/mol B) 440 k/J C) 117.9 k/J D) -41 kJ/K E) -440 kJ/K Given the following table of thermodynamic data. Complete the following sentence. The vaporization of TiCl_4 is _____ A) Spontaneous at all temperatures B) Spontaneous at low temperature and nonspontaneous at high temperature C) Nonspontaneous at low temperature and spontaneous at high temperature D) Nonspontaneous at all temperatures E) Not enough information given to draw a conclusion Which of the following has Delta G degree_f at 25 degree C? A) H_2O(l) B) H_2O(g) C) Na(s) D) O_3(g) E) O(g)

Explanation / Answer

33) del S= delSpdt - del S reac

del S= (2*89.62+18.83) - (330.73 + 2*32.68) = - 198.02 J/K

34) del S= (del H)/T

here, del S=(44*1000J/mol)/(100+273.15)K = 44000/373.15 = 117.9J/K

35) (A) as del G= del H - T(del S)= (-763.2+804.2) -T(354.9 - 221.9) = 41 -T(133).

A process is spontaneous if del G is negative.

thus, vaporization of TiCl4 is spontaneous if temperature in K is positive. In Kelvin scale, negative temperature is a theoretical situation.

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