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CHEM103 (DB425) Chemistry For Engineering
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Iron can be prepared by the reaction of Fe2O3 with carbon according to the equation:
2Fe2O3(s) + 3C(s) → 2CO2(g) + 4Fe(s)
If 401 g Fe2O3 and 40.0 g C are heated together, how many grams of iron could be produced?
Calculate the value of ΔGo for the decomposition of 1 mol of phosphorus trichloride to its constituent elements: 2 PCl3(g) → P2(g) + 3 Cl2(g)
Given the following standard heats of formation, calculate standard change in enthalpy for the reaction:
PbO2(s) + 2 H2SO4(aq) + Pb(s) → 2 PbSO4(s) + 2 H2O(l)
| Compound | Standard ΔHf (kJ/mol) |
| PbO2(s) | -277 |
| H2SO4(l) | -814 |
| PbSO4(s) | -920 |
| H2O(l) | -285 |
What is the concentration (M) of a NaCl solution prepared by dissolving 9.3 g of NaCl in sufficient water to give 350 mL of solution?
What is the coefficient of Al when the following equation is correctly balanced? Al + H2O → Al(OH)3 + H2
When 24.0 g of C5H12(g) is burned it warmed 40.0 kg of water by 0.200 °C. Find change in enthalpy in kJ/mol C5H12.
When a chemical equation is balanced, it will have a set of whole number coefficients which cannot be reduced to smaller whole numbers. What is the balancing coefficient for O2 when the following combustion reaction of a hydrocarbon is balanced? - C7H14 + - O2 → - CO2 + - H2O
How much heat (in kJ) is required to raise the temperature of 200.0 g of water from 25.0 °C to 39.5 °C. Use a molar heat capacity for water of 75.2 J·K-1·mol-1.
Given the equilibrium constants for the following equilibria at 25oC, H+(aq) + CO32-(aq) ⇋ HCO3-(aq) K = 2.1 x 1010 H+(aq) + HCO3- (aq) ⇋ H2CO3(aq) K = 2.4 x 106
calculate the equilibrium constant for the following reaction: H2CO3(aq) ⇋ 2H+(aq) + CO32-(aq)
What volume of 0.200M KMnO4 is required to prepare 50.0 mL of a 0.150 M solution?