1. A particular reaction has a H o value of -100 kJ and S o of -297 J/mol K at 2

Question

1. A particular reaction has a Ho value of -100 kJ and So of -297 J/mol K at 298 K. Assuming that Ho and So hardly change with temperature, determine the temperature in oC at which the spontaneity of this reaction changes.

2.Given the following data,

4 Al(s) + 3 O2(g) => 2 Al2O3(s) Go = -3,352

4 Al(s) + 3 MnO2(s) => 3 Mn(s) + 2 Al2O3(s) Go = -1,794

Determine Gfo for MnO2(s)

3. At 270 K, Go equals -44 kJ for the reaction, Cl2(g) + Br2(g) <=> 2 BrCl(g)

Calculate the value of ln K for the reaction at this temperature to one decimal place.

4. At a certain temperature, 310 K, Kp for the reaction,
F2(g) <=> 2 F(g), is 6.8 x 1018.
Calculate the value of DGo in kJ for the reaction at this temperature.

5. The value of Go for the reaction, N2(g) + 3 H2(g) <=> 2 NH3(g) is -32.90 kJ at 298 K.

Calculate the value of G in kJ at 298 K if the partial pressures of N2, H2 and NH3 are 8.553, 8.881, and 63 atm respectively.

Explanation / Answer

1) Ho value of -100 kJ and So of -297 J/mol K at 298 K

The reaction will be sponataneous if

Go < 0

We know that

Go = Ho - TS0

For Go = 0 = -100 +T x 0.297

T = 336.7

so Temperarture should be greater than 336.7 K

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