1 mole ethane, C2H6, is combusted in a reactor by using theoretical amounts of air. The products for this reaction are CO2(g) and H2O(g) at 25 °C. What is the heat of reaction? What are the exiting compositions of CO2(g), H2O(g), and N2(g)?  Using the computed heat of reaction, assume this amount is absorbed by the reactants, which are CO2(g), H2O(g), and the inert N2(g). What will be the final temperature of these gases?

(a) Consider the following chemical reaction: 3FE203(s) + CO(g) → 2Fe304(s) + CO2(g) AH° = ? Use the following thermochemical data to determine the enthalpy change of this reaction. (6) 2FE2O3 (s) AH° = -1652 kJ 4Fe(s) + 302(g) C(s,graphite) + ½O2(g) → CO(g) 3Fe(s) + 202 (g) → CO2(g) AH° = -110.5 kJ Fe304(s) C(s,graphite) + O2(g) AH° = -1117 kJ AH° = +395.5 kJ (b) What is the standard enthalpy of formation of carbon dioxide? (2)

The equilibrium constant for the reaction of nitrogen and hydrogen to give ammonia is 0.118 at 745 K. The balanced equilibrium equation is as follows: N2(g) + 3H₂(g) = 2NH3(g) What is Kp for this reaction at the same temperature? (R: 0.082 L atm/mol.K)

Q4) a) Explain why AStusion and AS,aporizaton are always positive? b) Natural gas is composed of 90% methane (CHa). As a heat source, methane is burned under the stream of O2. This reaction, namely combustion reaction, is given as follows : CH:(g) + 202(g) → CO2(g) +2H20(1) According to this reaction find out AA°reaction and AG°reaction at 298 K. s° (CO.) = 213.8 J/mol.K ; S° (H2O) = 70.0 J/mol.K ; S° (CH2) = 183.6 J/mol.K; s° (02) = 205.2 J/mol.K; AH°reaction = -890 kJ/mol. Assume that all reactants and products behave as an ideal gase.

Please I want to answer question 1 and question 2 because the second follows the first.

As reported in US Patent 4203923, cyclohexanone is an important chemical raw material in the production of nylon intermediates. The separation and purification section for cyclohexanone production usually done through a series of distillation units. Liquid mixture of cyclohexanone (1) and phenol (2) was reported to exist in equilibrium with its vapor at 144 °C (417.15K). The system conforms closely to Modified Raoult's Law. The mixture forms azeotrope at composition of 0.695. Iny;= Ax Iny,= Ax pgat = 75.20 kPa Pzat = 31.79 kPa A= 2.22 (a) Provide a sketch that clearly shows that the system exhibits azeotrope PatA pjat Pat and (b) State Paz and sketch a P-xy diagram of the system

You conduct the following reaction in the laboratory by mixing 30.0 g of NO: with excess water, Once the reaction is complete you determine that you actually produced 5.71 g of NO. What is the percent yield for the reaction? 3 NO:(g) + H:O(1) → 2 HNO (g) + NO(g)

At equilibrium at 425.6°C, a sample of cis-1-methyl- 2-ethyleyelopropane is 73.6% converted into the trans form: cis trans (a) Compute the equilibrium constant K for this reaction. (b) Suppose that 0.525 mol of the cis compound is placed in a 15.00-L vessel and heated to 425.6°C. Compute the equilibrium partial pressure of the trans compound.

The equilibrium constant with respect to temperature can be expressed for the reaction: Cyclohexane (g)! <--> methylcyclopentane (g) as: LnK = 4.814-2059/T. If placed to react 3 moles cyclohexane in a 5 liter container at a certain temperature and when equilibrium is reached, 8000 J of heat is released, Calculate the temperature of the container.

According to the reaction; MgO(s)+ CO2(g) MgCO3(s) (a) What is the enthalpy change of the reaction at 25 oC (b) What is the enthalpy change of the reaction at 406 oC (c) Assume that the reaction is completed in an adiabatic environment and the only product is MgCO3(s) at the end of reaction. Calculate the final temperature of MgCO3(s).