42) Which statement is FALSE? A) An exothermic reaction gives heat off heat to the surroundings. B) Enthalpy is the...
How much energy is evolved during the formation of 197 g of Fe, according to the reaction below? Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJ A. 964 kJ B. 1.52 x 103 kJ C. 3.02 x 103 kJ D. 482 kJ E. 8.40 x 103 kJ
5.) How much energy is evolved during the reaction of 4.00 moles of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) Hºrxn = -852 kJ/mole (remember, AH°rxn is referenced to the whole chemical equation as one mole unit)
5.) How much energy is evolved during the reaction of 4.00 moles of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) Hºrxn = -852 kJ/mole (remember, AH°rxn is referenced to the whole chemical equation as one mole unit)
C Using the heats of formation below, calculate the heat of reaction for the following reaction: CH4(g) + H2O(g) → C2H5OH(E) AH® (kJ/mol) C2H4(g) 52.26 H2O(g) -241.8 C2H5OH(E) -235.1 kJ d Using the heats of formation below, calculate the heat of reaction for the following reaction: Fe2O3(s) + 2Al(s) - A1203(s) + 2Fe(s) AH(kJ/mol) Fe2O3(s) -824.2 Al(s) 0 Al2O3(s) -1676 Fe(s) 0 KJ
Part A How much heat (in kilojoules) is evolved or absorbed in the reaction of 3.40 g of Fe2O3 with enough carbon monoxide to produce iron metal? Fe, 3 (s) + 3CO(g) + 2Fe(s) + 3C02(9) AH° = -24.8kJ. ΑΣΦ 9 = q= | kJ Submit Request Answer Part B Is the process exothermic or endothermic? The process is exothermic. The process is endothermic.
How much energy is evolved during the reaction of 48.7 g of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s), ΔH°rxn = -852 kJ
How much energy is evolved during the formation of 197 g of Fe, according to the reaction below? Fe2O3(s) + 2 Al(s) + A1203(s) + 2 Fe(s) AH®rxn - -852 kJ How do you find the correct answer to the problem question? DH(rxn of 197 g of Fe) = ratio of #mol from 197g of Fe in reaction / 2 mol of Fe in equation) x DHX of 2 mol of Fe). Amol from 197 sof is not known and...
Please help with these two questions :( 1. How much energy (in kJ) is evolved during the reaction of 76.9 g of Al, according to the reaction below? Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJ Assume that there is excess Fe2O3. 2. A 12.43 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity, C = 5.65 kJ/°C. C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(g) ΔH°rxn...
19) The thermite reaction given below is one of the most exothermic chemical reactions known. It is involved in a variety of industrial processes including welding. Iron (111) oxide is reduced at such a high temperature that the iron formed is in the liquid phase (MP = 1538*C). How much energy is evolved during the formation of 100.0g of Fe (55.85 g/mole)? Fe2O3(s) + 2Al(s) → Al2O3(s) +2Fe11 H rxn -852 kJ
. Use the equation below to calculate how much heat (in kJ) is evolved when 5.0 g of aluminium reacts with a stoichiometric amount of Fe2O3? 2 Al (s) + Fe2O3 (s) —>2 Fe (s) + Al2O3 (s) AH° = -852 kJ Determine the AHPrxn for the following reaction. {AH® (NH3) = -45.9 kJ/mol; AH°(O2) = 0; AH® (NO) = +91.3 kJ/mol; AH° (H2O) = -241.8 kJ/mol; 4 NH3 (g) + 5 O2 (g) — 4 NO (g) + 6...