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Practice Exercise 2
Given the following standard enthalpy change, use the standard enthalpies of formation in Table 5.3 to calculate the standard enthalpy of formation Of CuO(s):
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- Suppose 33 mL of 1.20 M HCl is added to 42 mL of a solution containing excess sodium hydroxide, NaOH, in a coffee-cup calorimeter. The solution temperature, originally 25.0C, rises to 31.8C. Give the enthalpy change, H, for the reaction: HCl(aq)+NaOH(aq)NaCl(aq)+H2O(l) Express the answer as a thermochemical equation. For simplicity, assume that the heat capacity and the density of the final solution in the cup are those of water. (In more accurate work, these values must be determined.) Also assume that the total volume of the solution equals the sum of the volumes of HCl(aq) and NaOH(aq).arrow_forwardercise 10.3 A 5.63-g sample of solid gold is heated from 21 to 32 °C. How much energy (in joules and calories) is required?arrow_forwardIron metal has a specific heat of 0.449 J/(g+ C). How much heat is transferred to a 5.00-g piece of iron, initially at 20.0C, when it is placed in a pot of boiling water? Assume that the temperature of the water is 100.0C and that the water remains at this temperature, which is the final temperature of the iron.arrow_forward
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- Issue 1Iron(III) oxide reacts with carbon monoxide to produce elemental iron and carbon dioxide. Determine the enthalpy change for this reaction using known enthalpies of formation. Fe2O3(s) + 3 CO(g) → 3 CO2(g) + 2 Fe(s) Issue 2Tetraphosphorus decaoxide, P4O10, is an acidic oxide. It reacts with water to produce phosphoric acid, H3PO4, in an exothermic reaction. P4O10(s) + 6 H2O(l) → 4 H3PO4(aq) ΔHorxn = -257.2 kJ a) Rewrite the thermochemical equation to include the enthalpy change as a term in the equation. b) How much energy is released from the reaction of 5.00 mol of P4O10 with excess water? Issue 4Find, using Hess's law, the overall enthalpy change of the reaction below. Determine whether the reaction is endothermic or exothermic. 2N2 + 5O2 → 2N2O5 Refer to the following reactions. 1) 2H2O → O2 + 2H2 ∆H= +572 kJ 2) N2O5 + H2O → 2HNO3 ∆H= -78 kJ 3) N2 + 3O2 + H2 → 2HNO3 ∆H= -349 kJ Issue 5The data in the table below was compiled for the following reaction. A + B → C + D…arrow_forwardSIMPLE ALGORITHM. Correct significant figures and rounding off (Conventional). 2. Given the following reactions Fe2O3(s) + 3CO(s) → 2Fe(s) + 3CO2(g) ΔH = -28.0 kJ 3Fe(s) + 4CO2(s) → 4CO2(g) + Fe3O4(s) ΔH = +12.5 kJ Determine the enthalpy of the reaction of Fe2O3 with CO: 3Fe2O3(s) + CO(g) → CO3(g) + 2Fe3O4(s).arrow_forwardTrial 1: Goldfish Mass of Empty Can (g) 12.715 g Mass of Can + Water (g) 112.831 g Mass of water (g) Mass of food + clip + foil + cork (g) BEFORE 5.285 g Mass of food + clip + foil + cork (g) AFTER 5.002 g Mass of Food Lost (g) INITIAL temperature (oC) 19.0 oC FINAL temperature (oC) 24.1 oC Temp Change (ΔT) How much energy (in Calories, ie. kcal) was produced by burning the Goldfish? (Specific Heat of water is 4.184 J/gC or 1.000 cal/gC)arrow_forward
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