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- When ethanol (CH;CH;OH) burns in oxygen, carbon dioxide and water are formed. (i) Write the equation which describes this reaction. (ii) Using the data below, calculate the value for AH° for the combustion of ethanol. AH; (CH;CH2OH(1)) = - 277.0 kJmol1 AH, (CO2(g)) = - 393.7 kJmol1 AH: (H2O()) = - 285.9 kJmol1The phase diagram for SO2 is shown here. (a) What doesthis diagram tell you about the enthalpy change in thereaction SO2(l) ---->SO2(g)? (b) Calculate the equilibriumconstant for this reaction at 100 °C and at 0 °C.(c) Why is it not possible to calculate an equilibrium constantbetween the gas and liquid phases in the supercriticalregion? (d) At which of the three points marked in reddoes SO2(g) most closely approach ideal-gas behavior?(e) At which of the three red points does SO2(g) behaveleast ideally?17D.1. (a) What is the specific heatof liquid water? (b) What is themolar heat capacity of liquid water?(c) What is the heat capacity of 185 gof liquid water? (d) How many kJ ofheat are needed to raise thetemperature of 10.00 kg of liquidwater from 24.6 °C to 46.2 °C?
- Ammonium sulfate, (NH,),SO4, is used as a fire retardant and wood preservative; it is prepared industrially by the highly exothermic reaction of gaseous ammonia with sulfuric acid: 2 NH, (g) + H,SO,(aq)→ (NH, ),SO, (s) The value of AH°, ammonium sulfate (in kilojoules per mole). is -179.4 kJ/g H, SO. Use the data in Table T1 to calculate the standard enthalpy of formation of rxnC6H12O6(aq) + 6O2(g) 6CO2(g) + 6H2O(l)ΔH = –2802.7 kJ mol –1a) Write an expression for the equilibrium constant for this reaction.b) At equilibrium, the concentration of the reactants and products are determined as [CO2] = 0.30 M, [O2] = 0.040 M and [C6H12O6] = 0.065 M. Determine the value of the equilibrium constant (Kc) and predict the whether the products or reactants will be favoured at equilibrium.c) Given that the concentrations of the reactants and products at a particular time are [CO2] = 0.65 M, [O2] = 0.020 M and [C6H12O6] = 0.055 M, determine the reaction quotient (Qc). Compare the Kc and Qc values and predict the favoured direction of the reaction.d) Explain the effect on equilibrium of:i) Increasing temperatureii) Increasing pressureiii) Decreasing the concentration of oxygeniv) Increasing the concentration of carbon dioxidev) Adding a catalystJO(g) at high (g), with the gases treated as perfect. E6A.5(b) Write the equilibrium constant for the reaction CH₂(g) + 3 Cl₂(g) ⇒CHCl,(1) + 3 HCl(g), with the g CHC1₂(1) + 3 HCl(g), with the gases treated as perfect. A diiw 1000 ABOUT E6A.6(a) Use data founde Resource section to decide which of
- Certain amount of pure charcoal (carbon) has to be burnt with supplied natural air. Process engineer allowed exact amount of air required to burn the entire charcoal completely to carbon dioxide. Carbon has no reaction with nitrogen gas present in the air. In the reaction outlet if 50 kg of carbon dioxide gas was found, calculate the amount of charcoal and air used. (12C, 16O, 14N).Given the dissociation reaction, Br2(g) = 2 Br(g), AH = + 112 kJ mol^ - 1 molecular bromine is 35 per cent dissociated at 1600 K and 1.00 bar at equilibrium. Calculate the equilibrium constant, K at 25\deg C. At what temperature would the reaction mixture need to be to turned off, ~ K = 10^-5?Estimate the temperature at which (a) CaCO3 decomposes spontaneouslyand (b) CuSO4.5H2O undergoes dehydration .
- how did they arrive with the answer HCI (g) 5 H* (aq) + Cl- (aq) ΔG ΔΗ-TAS = (-75.15 x 103 Jmol-1) – (298.15 K) (-131.5 JK-1mol-1) AG° = - 35.94 kJ mol-1At 3000K and 1 atm pressure, CO2 is 40% dissociated into CO and O2. (a)What will be the degree of dissociation if the pressure is raised to 2 atm? (b)What will be the degree of dissociation when a mixture of 70% CO2 and 30% O2 is heated into 2500 K, the pressure being 3 atm?Consider The Following Reaction: CaCO3(S) + 2HCl(Aq) = CaCl2(Aq) + H2O(L) + CO2(G) Write down the quation of the equilibrium constant kc for this reaction