1. 2 mol of Hg(g) is combusted in a fixed volume bomb calorimeter with excess of...

  

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1. 2 mol of Hg(g) is combusted in a fixed volume bomb calorimeter with excess of O2 at 298 K and 1 atm into HgO(s). During the reaction, temperature increases from 298.0 K to 312.8 K. If heat capacity of the bomb calorimeter and enthalpy of formation of Hg(g) are 20.00 kJ K-1 and 61.32 kJ mol-1 at 298 K, respectively, the calculated standard molar enthalpy of formation of HgO(s) at 298 K is X kJ mol-1. The value of |X| is [Given: Gas constant R = 8.3 J K-1 mol-1] 2. The reduction potential (E, in V) of MnO4(aq)/Mn(s) is. [Given: EMnO3(aq)/MnO = 1.68 V; E = 1.21 V; E = -1.03 V] (MnO4(aq)/MnO2(s)) (MnO2(s)/Mn2+(aq)) (Mn2+(aq)/Mn(s)) 1. 2 mol of Hg(g) is combusted in a fixed volume bomb calorimeter with excess of O2 at 298 K and 1 atm into HgO(s). During the reaction, temperature increases from 298.0 K to 312.8 K. If heat capacity of the bomb calorimeter and enthalpy of formation of Hg(g) are 20.00 kJ K-1 and 61.32 kJ mol-1 at 298 K, respectively, the calculated standard molar enthalpy of formation of HgO(s) at 298 K is X kJ mol-1. The value of |X| is [Given: Gas constant R = 8.3 J K-1 mol-1] 2. The reduction potential (E, in V) of MnO4(aq)/Mn(s) is. [Given: EMnO3(aq)/MnO = 1.68 V; E = 1.21 V; E = -1.03 V] (MnO4(aq)/MnO2(s)) (MnO2(s)/Mn2+(aq)) (Mn2+(aq)/Mn(s))