Question

2. The combustion of 3.4554 g of methylhydrazine (CH3NH-NH2, molar mass 46.072 g/mol) increases the temperature of a calorimeter from 25.00 °C to 37.55 °C. In a separate combustion experiment the heat capacity of the calorimeter system was measured to be 7.794 kJ/K. The combustion reaction is as follows. CH6N2(l) + 5/2 O2(g) ? N2 (g) + CO2 (g) + 3 H2O (l) The following data may be useful: ?fH0[CO2 (g)] = -393.15 kJ/mol ?fH0[H2O (l)] = -285.83 kJ/mol ?fH0[H2O (g)] = -241.818 kJ/mol i) What is the molar heat of combustion of methylhydrazine: a) -97.81 kJ/mol b) -1,320.2 kJ/mol c) -2,544 kJ/mol d) -1,305.4 kJ/mol e) -1,304.2 kJ/mol f) -33,520 kJ/mol ii) Calculate the standard enthalpy of formation of methylhydrazine a) - 54.7 kJ/mol b) +186.7 kJ/mol c) + 54.7 kJ/mol d) -1,250.6 kJ/mol e) + 53.6 kJ/mol f) + 1293 kJ/mol

          2. The combustion of 3.4554 g of methylhydrazine (CH3NH-NH2, molar mass 46.072 g/mol) increases the temperature of a calorimeter from 25.00 °C to 37.55 °C. In a separate combustion experiment the heat capacity of the calorimeter system was measured to be 7.794 kJ/K. The combustion reaction is as follows.

CH6N2(l) + 5/2 O2(g) ? N2 (g) + CO2 (g) + 3 H2O (l)

The following data may be useful: ?fH0[CO2 (g)] = -393.15 kJ/mol ?fH0[H2O (l)] = -285.83 kJ/mol
?fH0[H2O (g)] = -241.818 kJ/mol

i) What is the molar heat of combustion of methylhydrazine:
a) -97.81 kJ/mol b) -1,320.2 kJ/mol c) -2,544 kJ/mol
d) -1,305.4 kJ/mol e) -1,304.2 kJ/mol f) -33,520 kJ/mol

ii) Calculate the standard enthalpy of formation of methylhydrazine
a) - 54.7 kJ/mol b) +186.7 kJ/mol c) + 54.7 kJ/mol
d) -1,250.6 kJ/mol e) + 53.6 kJ/mol f) + 1293 kJ/mol

2. The combustion of 3.4554 g of methylhydrazine (CH3NH-NH2, molar mass 46.072 g/mol) increases the temperature of a calorimeter from 25.00 °C to 37.55 °C. In a separate combustion experiment the heat capacity of the calorimeter system was measured to be 7.794 kJ/K. The combustion reaction is as follows.

CH6N2(l) + 5/2 O2(g) ? N2 (g) + CO2 (g) + 3 H2O (l)

The following data may be useful: ?fH0[CO2 (g)] = -393.15 kJ/mol ?fH0[H2O (l)] = -285.83 kJ/mol
?fH0[H2O (g)] = -241.818 kJ/mol

i) What is the molar heat of combustion of methylhydrazine:
a) -97.81 kJ/mol b) -1,320.2 kJ/mol c) -2,544 kJ/mol
d) -1,305.4 kJ/mol e) -1,304.2 kJ/mol f) -33,520 kJ/mol

ii) Calculate the standard enthalpy of formation of methylhydrazine
a) - 54.7 kJ/mol b) +186.7 kJ/mol c) + 54.7 kJ/mol
d) -1,250.6 kJ/mol e) + 53.6 kJ/mol f) + 1293 kJ/mol

Added by Amber P.

Question

Please give Ace some feedback