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How does changing the volume affect the equilibrium position of a chemical reaction? Provide an example of a reaction and calculate the new equilibrium concentrations when the volume is decreased by a certain factor.

asked Feb 3 in Chemical equilibrium by QuincyBoake8 (450 points)

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Calculate the standard enthalpy change for the reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) to form sodium chloride (NaCl) and water (H2O) when 50.0 mL of 1.0 M HCl reacts with 50.0 mL of 1.0 M NaOH at 25°C.

asked Feb 3 in Chemical thermodynamics by JudithWooten (490 points)

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Calculate the standard Gibbs free energy change (ΔG°) for the reaction below at 298 K:2NO(g) + O2(g) → 2NO2(g)Given:ΔG°f(NO2(g)) = -51.29 kJ/molΔG°f(NO(g)) = 86.67 kJ/molΔG°f(O2(g)) = 0 kJ/mol

asked Feb 3 in Physical Chemistry by TrevorPerdri (430 points)

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Calculate the standard enthalpy change for the reaction 2H2(g) + O2(g) ⟶ 2H2O(g), given that the standard enthalpies of formation of H2(g), O2(g), and H2O(g) are 0 kJ/mol, 0 kJ/mol, and -242 kJ/mol, respectively.

asked Feb 3 in Chemical thermodynamics by PattyIsom30 (190 points)

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Calculate the standard enthalpy change (∆H°) for the reaction between 25.0 mL of 0.100 M HCl and 25.0 mL of 0.100 M NaOH at 25°C. The density of each solution is 1.00 g/mL and the heat capacity of the solution is 4.18 J/g·°C. The reaction takes place in a calorimeter, and the temperature increase is measured to be 8.47°C.

asked Feb 3 in Chemical thermodynamics by CarmaU145909 (290 points)

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Calculate the standard enthalpy of formation for hydrogen peroxide (H2O2) at 298 K, given that the standard enthalpy change of formation for water (H2O) is -285.8 kJ/mol and the standard enthalpy change of formation for oxygen gas (O2) is 0 kJ/mol.

asked Feb 3 in Chemical thermodynamics by HamishChappe (330 points)

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Calculate the standard free energy change for the following redox reaction:2HgO(s) → 2Hg(l) + O2(g)Given: ΔG°f (HgO) = -90.83 kJ/molΔG°f (Hg) = 0 kJ/mol ΔG°f (O2) = 0 kJ/mol.

asked Feb 3 in Chemical thermodynamics by EdwinCamidge (450 points)

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Can the chemical modification of a polymer affect its optical properties and if so, how can we design a polymer with unique optical properties for use in advanced optical materials?

asked Feb 3 in Polymer Chemistry by ThaliaEsmond (390 points)

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Calculate the standard free energy change for the following redox reaction under standard conditions:2 Fe3+ (aq) + H2 (g) → 2 Fe2+ (aq) + 2 H+ (aq)Given: Standard reduction potential of Fe3+ / Fe2+ = -0.771 V Standard reduction potential of H+ / H2 = 0.00 V

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

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Calculate the standard enthalpy and standard entropy change at 298 K for the following reaction: 2Fe(s) + 3/2O2(g) → Fe2O3(s) Given that the standard enthalpies of formation for Fe(s), O2(g), and Fe2O3(s) are 0 kJ/mol, 0 kJ/mol, and -826 kJ/mol respectively. Also, the standard molar entropy of Fe2O3(s) is 87.4 J/K/mol.

asked Feb 3 in Inorganic Chemistry by Jefferson313 (490 points)

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Calculate the standard enthalpy change for the following reaction involving liquids at 298 K: C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l)Given the standard enthalpies of formation of C2H5OH(l), CO2(g) and H2O(l) are −277.6 kJ/mol, −393.5 kJ/mol and −285.8 kJ/mol respectively.

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

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Calculate the standard enthalpy change for the following reaction at 298 K:Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)

asked Feb 3 in Quantum Chemistry by HectorShapir (730 points)

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Calculate the standard entropy change for the reaction: 2SO3(g) + O2(g) → 2SO4(g) Given the following standard entropies of formation: ΔS°f SO3(g) = 256.2 J/K mol ΔS°f O2(g) = 205.0 J/K mol ΔS°f SO4(g) = 296.8 J/K mol

asked Feb 3 in Inorganic Chemistry by WBFCharli644 (270 points)

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Consider the electrochemical cell with the following half-cell reactions: Fe3+ (aq) + e- → Fe2+ (aq) E° = +0.771 V and Cd2+ (aq) + 2e- → Cd (s) E° = -0.403 V What is the overall cell potential, Ecell, under standard conditions? Which species will be reduced at the cathode? Which electrode is the anode? Justify your choices using the given standard reduction potentials.

asked Feb 3 in ElectroChemistry by EdwardTier7 (390 points)

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Design a biodegradable polymer that can be used as a sustainable alternative to single-use plastic bags, and provide a detailed synthesis route for its production.

asked Feb 3 in Polymer Chemistry by XTFAnderson (290 points)

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1 answer 41 views

Calculate the standard enthalpy change for the neutralization reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH), given the appropriate thermochemical equations and the following information:- Heat evolved during the reaction, Q = -58.35 kJ/mol- Moles of HCl used, n(HCl) = 0.05 mol- Concentration of NaOH solution, c(NaOH) = 2 M- Volume of NaOH solution used, V(NaOH) = 25.0 mL (assuming density of 1.00 g/mL)Show your calculations and include units in your final answer.

asked Feb 3 in Chemical thermodynamics by RetaStoddard (570 points)

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Calculate the standard entropy change for the following reaction at 298 K:CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l) Given the standard entropies of CH4(g), O2(g), CO2(g), and H2O(l) are 186.26 J/K/mol, 205.03 J/K/mol, 213.74 J/K/mol, and 69.95 J/K/mol respectively.

asked Feb 3 in Chemical thermodynamics by DolliePalmer (530 points)

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Calculate the standard enthalpy change for the vaporization reaction of 2.00 moles of water at 100°C and 1 atm pressure, given that the molar enthalpy of vaporization of water is 40.7 kJ/mol.

asked Feb 3 in Chemical thermodynamics by Madelaine706 (330 points)

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Calculate the standard electrode potential for the redox reaction where Ag(s) is oxidized by Cu2+(aq) to form Ag+(aq) and Cu(s) given that the standard reduction potential for Ag+(aq) + e- → Ag(s) is 0.80 V and for Cu2+(aq) + 2e- → Cu(s) is 0.34 V.

asked Feb 3 in Chemical thermodynamics by SheilaCrawfo (420 points)

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Calculate the standard enthalpy change for the dissolution of 10 g of NaOH in 100 mL of water at 25°C if the molar enthalpy of dissolution is -44.5 kJ/mol.

asked Feb 3 in Chemical thermodynamics by Eduardo04095 (490 points)

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