A 2.20 g sample of the Ethane C2H6 gas was mixed with excess
oxygen gas and a combustion reaction occurred to obtain water in
liquid aggregate and carbon dioxide state. The combustion reaction
occurred at a constant calorimeter under standard conditions.
After the reaction was completed, the temperature in the
calorimeter rose by 1.3K. The heat capacity of the calorimeter is
88.8 kJ / K.
1. Write a balanced response to the burning process that took
place.
2. Consider the change in standard enthalpy,, ∆H for a 1 molar
reaction of ethane. Show calculations.
3. Explain how you would calculate [(Hf∆ [C2H6 (g) given you values
of:
[(Hf∆ [CO2 (g
[(Hf∆ [H2O (g
Numerical calculations are not required.
4. Determine what the missing data is to calculate the change in
the fire enthalpy,
Hc∆ of ethane at 100 C?
5. Is a difference between ∆Ho and ∆Uo expected for the reaction
formulated in section a? Explain
A 2.20 g sample of the Ethane C2H6 gas was mixed with excess oxygen gas and...
The standard enthalpy of combustion of ethane gas, C2H6 is −1560 kJ·mol−1. Given that ∆Hf° CO2, (g) = −394 kJ·mol−1, and ∆Hf° H2O, (l) = −286 kJ·mol−1. Calculate ∆Hf° C2H6 (g).
The gas ethane, C2H6(g), can be used in welding. When ethane is burned in oxygen, the reaction is: 2 C2H6(g) + 7 O2(g)4 CO2(g) + 6 H2O(g) (a) Using the following data, calculate ΔH° for this reaction. ΔH°f kJ mol-1: C2H6(g) = -84.0 ; CO2(g) = -393.5 ; H2O(g) = -241.8 ΔH° = kJ (b) Calculate the total heat capacity of 4 mol of CO2(g) and 6 mol of H2O(g), using CCO2(g) = 37.1 J K-1 mol-1 and CH2O(g) =...
Ethane gas (C2H6) reacts with oxygen gas according to the reaction below 2C2H6 (g) + 7O2 (g) > 4CO2 (g) + 6H2O (g) In a particular study, the rate of consumption of ethane gas (C2H6) is found to be 0.25 Ms-1 what is the rate of formation of co2?
The combustion reaction of ethane is as follows. C2H6(g) + 7/2 O2(g) → 2 CO2(g) + 3 H2O(l) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. reaction (1): C(s) + O2(g) → CO2(g) ΔH = −393.5 kJ/mol reaction (2): H2(g) + 1/2 O2(g) → H2O(l) ΔH = −285.8 kJ/mol reaction (3): 2 C(s) + 3 H2(g) → C2H6(g) ΔH = −84.0 kJ/mol
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