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Calculate the standard enthalpy change for the reaction: NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l) Given the following information: ΔHf° [NaOH(aq)] = -469.1 kJ/mol ΔHf° [HCl(aq)] = -167.2 kJ/mol ΔHf° [NaCl(aq)] = -407.3 kJ/mol ΔHf° [H2O(l)] = -286 kJ/mol

asked Feb 3 in Chemical thermodynamics by LinneaZox85 (370 points)

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Calculate the standard enthalpy change for the reaction: CuSO4 (aq) + 4NH3 (aq) -> Cu(NH3)4SO4 (aq) given that the standard enthalpy changes of formation for CuSO4 (aq) and NH3 (aq) are -771.5 kJ/mol and -46.19 kJ/mol respectively, and the standard enthalpy change of formation for Cu(NH3)4SO4 (aq) is -2130.4 kJ/mol.

asked Feb 3 in Chemical thermodynamics by Juliet26542 (190 points)

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Calculate the standard enthalpy change for the reaction: CH4(g) + 2O2(g) -> CO2(g) + 2H2O(g) Given the necessary bond enthalpies are: C-H = 411 kJ/molO=O = 495 kJ/molO-H = 463 kJ/molC=O = 799 kJ/mol.

asked Feb 3 in Quantum Chemistry by ChristineR12 (430 points)

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Calculate the standard enthalpy change for the reaction: CH3OH (l) + 3/2 O2 (g) -> CO2 (g) + 2H2O (l) given the standard enthalpies of formation for CH3OH (l), CO2 (g) and H2O (l) as -238.6 kJ/mol, -393.5 kJ/mol and -285.8 kJ/mol respectively.

asked Feb 3 in Chemical thermodynamics by JensW5136048 (430 points)

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Calculate the standard enthalpy change for the reaction: C6H12O6 (s) + 6O2 (g) → 6CO2 (g) + 6H2O (l)Given the following standard enthalpies of formation: ΔHf(C6H12O6 (s)) = -1273 kJ/molΔHf(CO2 (g)) = -393.5 kJ/molΔHf(H2O (l)) = -285.8 kJ/mol

asked Feb 3 in Chemical thermodynamics by MargieSelph6 (370 points)

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Calculate the standard enthalpy change for the reaction: 2NaOH (s) + H2SO4 (aq) → Na2SO4 (aq) + 2H2O (l)given that the standard enthalpy of formation of Na2SO4 (aq) is -1385 kJ/mol, and the standard enthalpies of formation of NaOH (s), H2SO4 (aq) and H2O (l) are -425 kJ/mol, -814 kJ/mol and -286 kJ/mol respectively.

asked Feb 3 in Chemical thermodynamics by EileenRubin0 (510 points)

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Calculate the standard enthalpy change for the reaction: 2H2(g) + O2(g) → 2H2O(l)Given the standard enthalpies of formation are: ΔHf°(H2O(l)) = -285.8 kJ/mol ΔHf°(H2(g)) = 0 kJ/mol ΔHf°(O2(g)) = 0 kJ/mol Assume all reactants and products are at standard state conditions.

asked Feb 3 in Chemical thermodynamics by TressaSteigr (390 points)

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Calculate the standard enthalpy change for the reaction: 2H2(g) + O2(g) --> 2H2O(l)Given the following enthalpies of formation: ∆Hf°(H2O, l) = -285.8 kJ/mol ∆Hf°(H2, g) = -241.8 kJ/mol ∆Hf°(O2, g) = 0 kJ/mol

asked Feb 3 in Chemical thermodynamics by AlannahMuntz (510 points)

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Calculate the standard enthalpy change for the reaction: 2Fe(s) + 3/2 O2(g) -> Fe2O3(s) given that the standard enthalpy of formation for Fe2O3(s) is -824.2 kJ/mol and that of Fe(s) is 0 kJ/mol.

asked Feb 3 in Chemical thermodynamics by HildegardeL3 (150 points)

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Calculate the standard enthalpy change for the reaction: 2C2H5OH(l) + 9O2(g) -> 6CO2(g) + 8H2O(l) given that the standard enthalpy of formation for C2H5OH(l) is -278 kJ/mol, for CO2(g) is -394 kJ/mol and for H2O(l) is -286 kJ/mol.

asked Feb 3 in Chemical thermodynamics by OrlandoBosle (510 points)

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Calculate the standard enthalpy change for the reaction: [Cu(H2O)6]2+(aq) + 2NH3(aq) → [Cu(NH3)4(H2O)2]2+(aq) + 4H2O(l)given the following information: ΔHf° [Cu(H2O)6]2+(aq) = -203.2 kJ/molΔHf° [Cu(NH3)4(H2O)2]2+(aq) = -368.5 kJ/molΔHf° H2O(l) = -285.8 kJ/molΔHf° NH3(aq) = -80.8 kJ/mol

asked Feb 3 in Chemical thermodynamics by LawrenceDyal (310 points)

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Calculate the standard enthalpy change for the reaction: [Co(H2O)6]2+(aq) + 4Cl-(aq) → [CoCl4]2-(aq) + 6H2O(l) Given the following information:• ΔH°f of [Co(H2O)6]2+ is 32.3 kJ/mol • ΔH°f of [CoCl4]2- is -341.8 kJ/mol • ΔH°f of H2O(l) is -285.8 kJ/mol • The ΔH°f of Cl- is taken as zero

asked Feb 3 in Chemical thermodynamics by JesusBittner (370 points)

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Calculate the standard enthalpy change for the reaction where 50 ml of 0.1 M hydrochloric acid reacts with 50 ml of 0.1 M sodium hydroxide solution. The temperature change observed during the reaction was 5°C and the specific heat capacity of the solution is 4.18 J/g°C.

asked Feb 3 in Chemical thermodynamics by Lillie851485 (430 points)

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Calculate the standard enthalpy change for the reaction where 3 moles of hydrogen gas react with 1 mole of nitrogen gas to form 2 moles of ammonia gas. Given the following thermochemical equation: N2(g) + 3 H2(g) → 2 NH3(g) ΔH° = −92.4 kJ/mol

asked Feb 3 in Chemical thermodynamics by PatrickSherr (470 points)

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Calculate the standard enthalpy change for the reaction where 250 mL of 2M HCl is mixed with 500 mL of 1M NaOH, assuming that the specific heat capacity of the resulting solution is 4.18 J/g°C and the density of the solution is 1.00 g/mL. (Hint: The balanced chemical equation for the reaction is HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l))

asked Feb 3 in Chemical thermodynamics by JerilynNabor (430 points)

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Calculate the standard enthalpy change for the reaction that occurs when 50 grams of ice at -10°C is heated to water at 25°C. The molar enthalpy of fusion of ice is 6.01 kJ/mol, and the specific heat capacity of water and ice are 4.184 J/g°C and 2.09 J/g°C, respectively. (Assume that the entire sample of ice is converted to water and that no heat is lost to the surroundings.)

asked Feb 3 in Chemical thermodynamics by FlorentinaRo (370 points)

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Calculate the standard enthalpy change for the reaction that occurs when 4.50 grams of magnesium oxide reacts with excess hydrochloric acid, given the following information:2HCl(aq) + MgO(s) → MgCl2(aq) + H2O(l) ΔH = -120.3 kJ/molMolar mass of MgO = 40.31 g/molRound your answer to two decimal places.

asked Feb 3 in Chemical thermodynamics by LettieMcclel (390 points)

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Calculate the standard enthalpy change for the reaction of the coordination compound Cu(NH3)4SO4 with excess NaOH to form Cu(OH)2(s), NH3(g), Na2SO4(aq), and H2O(l) at a constant pressure of 1 atm and a temperature of 25°C.

asked Feb 3 in Chemical thermodynamics by CathrynShiel (430 points)

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Calculate the standard enthalpy change for the reaction of the combustion of liquid ethylene glycol $(C_2H_6O_2)$ when 500g of the compound is burned completely with excess oxygen gas, given the enthalpies of formation of $CO_2$ (-393.5 kJ/mol), $H_2O$ (-285.8 kJ/mol), and $C_2H_6O_2$ (-694.3 kJ/mol).

asked Feb 3 in Chemical thermodynamics by LashondaBurc (510 points)

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Calculate the standard enthalpy change for the reaction of the combustion of 1 mole of liquid ethanol (C2H5OH) at 298K and 1 atm. The balanced chemical equation for the reaction is: C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l)Given:ΔHf°(C2H5OH(l)) = -277.7 kJ/molΔHf°(CO2(g)) = -393.5 kJ/molΔHf°(H2O(l)) = -285.8 kJ/molΔHf°(O2(g)) = 0 kJ/mol

asked Feb 3 in Chemical thermodynamics by PedroShuler0 (430 points)

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