A 2.20 g sample of the Ethane C2H6 gas was mixed with excessoxygen gas and a combustion reaction occurred to obtain water inliquid aggregate and carbon dioxide state. The combustion reactionoccurred at a constant calorimeter under standard conditions.
After the reaction was completed, the temperature in thecalorimeter rose by 1.3K. The heat capacity of the calorimeter is88.8 kJ / K.
1. Write a balanced response to the burning process that tookplace.
2. Consider the change in standard enthalpy, ∆H for a 1 molarreaction of ethane. Show calculations.
3. Explain how you would calculate ∆Hf[C2H6(g)] given you values ​​of:
∆Hf [CO2(g)] and ∆Hf[H2O(l)]
Numerical calculations are not required.
4. Determine what the missing data is to calculate the change inthe fire enthalpy,
∆Hc of ethane at 100 C?
5. Is a difference between ∆Ho and ∆Uoexpected for the reaction formulated in section a? Explain
