1. A particular reaction has a ÎHo value of -100 kJ and ÎSo of -297 J/mol K at 298 K. Assuming that ÎHo and ÎSo 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) ÎGo = -3,352
4 Al(s) + 3 MnO2(s) => 3 Mn(s) + 2 Al2O3(s) ÎGo = -1,794
Determine ÎGfo for MnO2(s)
3. At 270 K, ÎGo 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 ÎGo for the reaction, N2(g) + 3 H2(g) <=> 2 NH3(g) is -32.90 kJ at 298 K.
Calculate the value of ÎG in kJ at 298 K if the partial pressures of N2, H2 and NH3 are 8.553, 8.881, and 63 atm respectively.
1. A particular reaction has a ÎHo value of -100 kJ and ÎSo of -297 J/mol K at 298 K. Assuming that ÎHo and ÎSo 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) ÎGo = -3,352
4 Al(s) + 3 MnO2(s) => 3 Mn(s) + 2 Al2O3(s) ÎGo = -1,794
Determine ÎGfo for MnO2(s)
3. At 270 K, ÎGo 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 ÎGo for the reaction, N2(g) + 3 H2(g) <=> 2 NH3(g) is -32.90 kJ at 298 K.
Calculate the value of ÎG in kJ at 298 K if the partial pressures of N2, H2 and NH3 are 8.553, 8.881, and 63 atm respectively.
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