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Iron can be extracted from haematite, Fe2O3, using either C or CO2 as the reducing agent.
The reactions are shown below.
Fe2O3(s) + 3 C(s) → 2 Fe(s) + 3 CO(g) ΔH = +492.7 kJ /mol
Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) ΔH = - 24.8 kJ/mol
Substance S° (J/ K·mol)
Fe2O3 (s) 87.4
Fe (s) 27.3
C (s) 5.7
CO (g) 197.6
CO2 (g) 213.6
Use available data given to:
1. Calculate the minimum temperature at which reduction with carbon is feasible
2. Prove by calculation that reduction with carbon monoxide is feasible at all temperatures
Determine the pH of a 0.20 M NH3 solution.
1. Determine S for the reaction:
SO3(g) + H2O(l) —> H2SO4(l)
Given: S°(J/K·mol): 256.2 69.9 156.9
2. Calculate S for the reaction
SO2(s) + NO2(g) —> SO3(g) + NO(g)
Given: S°(J/K·mol): 248.5 240.5 256.2 210.6
3. Calculate S at 25C for the reduction of given these absolute entropies:
2PbO(s) + C(s) —> 2Pb(s) + CO2(g)
Given: S°(J/K·mol): 69.54 5.7 64.89 213.6
Predict whether the entropy change of the system in each of the following is positive or negative
1. O2(g) —> 2O(g)
2. N2 (g, 10 atm) —> N2 (g, 1atm).
3. 6CO2(g) + 6H2O(g) —> C6H12O6(g) + 6O2(g).
4. 2 H2 (g) + O2 (g) —> 2 H2O (l)
5. NH4Cl (s) —> NH3(g) + HCl (g)
A mixture of gases consists of N2, O2, H2 and F2. The total pressure of the mixture is 511.56 kPa. The pressure of the N2 is 584 mm Hg, the pressure of the O2 is 196 kPa and the pressure of the H2 is standard pressure. What is the pressure of the F2 (in mm Hg)?
Given the equation N2(g)+3H2(g)--->2NH3(g) if ∆H=-92.2kJ and ∆S=-0.1987kJ/K, what is ∆G for reaction at 475°C and at 5°C? Provide the answer in kJ. In each case, is the reaction spontaneous?
Can an e be described by the following set of quantum numbers? If not indicate which of the quantum numbers has a value that is not valid: n=2, £=1, ml= -1, Ms=+½
If 15.65 mL of aq HCl is required to neutralize 20.00mL of the sodium carbonate solution from question 4 above ,what is the molarity of the aq HCl ? Show all your steps in your calculations below as set out below
Calculate the number of moles of Na2CO3 (standard solution) used in the titration
Using the balanced reaction equation find the number of moles of HCl that reacted
Calculate the molarity of HCl solution
A sample of 0.892 g of potassium chloride (KCl) is dissolved in 54.6 g of water (H2O). Determine the percent mass of KCl in the solution and its molality if the molar mass of KCl is 74.5513 grams per mole.
A sample of 0.892 g of potassium chloride (KCl) is dissolved in 54.6 g of water. What is the percent by mass of KCl in the solution?
A sample of 0.892 g of potassium chloride (KCl) is dissolved in 54.6 g of water. What is the percent by mass of KCl in the solution?
The density of a 2.45 M aqueous solution of methanol (CH3OH) is 0.976 g/mL. What is the molality of the solution? The molar mass of methanol is 32.04g.
You have ice at 263 K (-10.00°C) and 1.0 atm. What could you do to make the ice sublime
