Recent questions in Chemistry

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Calculate the equilibrium constant (Kc) for the following gas-phase reaction at 298 K: N2(g) + O2(g) ⇌ 2NO(g) where the initial concentrations of N2, O2, and NO are 0.100 M, 0.050 M, and 0.000 M respectively.

asked Jan 23 in Chemical equilibrium by AguedaMuniz6 (490 points)

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Calculate the equilibrium constant (Kc) for the following chemical reaction at 25°C, given that the concentrations of reactant A and product B are 0.05 M and 0.10 M, respectively:A(s) + 2B(g) ⇌ 3C(g) The equilibrium concentration of compound C is found to be 0.15 M.

asked Jan 23 in Chemical thermodynamics by RaymonSchmid (630 points)

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Calculate the equilibrium constant (Kc) at 298 K for the reaction: 2 NH3(g) ⇌ N2(g) + 3 H2(g) given that the equilibrium concentration of NH3 is 0.20 M, N2 is 0.025 M, and H2 is 0.060 M.

asked Jan 23 in Chemical thermodynamics by HeikeCranfor (530 points)

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Calculate the equilibrium constant (Kc) at 25°C for the following redox reaction involving a weak oxidizing agent: H2O2(aq) + 2I^-(aq) + 2H^+(aq) ⇌ I2(aq) + 2H2O(l)

asked Jan 23 in Chemical equilibrium by HildaDoyne30 (510 points)

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Calculate the equilibrium constant (K) of the electrochemical reaction below at 298K:Fe(s) + Cu2+(aq) ⇌ Fe2+(aq) + Cu(s) Given that at standard state (1 atm and 298K) the standard reduction potentials of Fe2+(aq)/Fe(s) and Cu2+(aq)/Cu(s) are -0.44 V and +0.34 V, respectively.

asked Jan 23 in ElectroChemistry by SkyeVillasen (610 points)

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1 answer 43 views

Calculate the equilibrium constant (K) of the electrochemical reaction below at 25°C: 2AgCl(s) + H2(g) <--> 2Ag(s) + 2HCl(aq) Given: E°AgCl/Ag = 0.22 V E°HCl/H2 = 0.00 V Kw = 1.0 x 10^-14 at 25°C Standard Hydrogen Electrode (SHE) has E° = 0.00 V

asked Jan 23 in ElectroChemistry by StefanieWhip (350 points)

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1 answer 52 views

Calculate the equilibrium constant (K) for the reaction that occurs when a nickel electrode is placed in a solution containing 1.0 M of nickel ions and 1.0 M of copper ions. The nickel electrode was placed in the solution, and the cell potential was measured to be 0.21 V at 25 °C.

asked Jan 23 in ElectroChemistry by JerrodLeidig (190 points)

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1 answer 51 views

Calculate the equilibrium constant (K) for the reaction between copper and silver ions in a galvanic cell at room temperature (25°C), given the following half-reactions and their respective reduction potentials:Cu2+ (aq) + 2e- → Cu (s) E°red = +0.34 VAg+ (aq) + e- → Ag (s) E°red = +0.80 VAlso, if the cell is constructed with a copper electrode and a silver electrode, which electrode will be the cathode and which will be the anode?

asked Jan 23 in ElectroChemistry by LakeishaA172 (500 points)

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1 answer 57 views

Calculate the equilibrium constant (K) for the formation of the complex ion [Fe(SCN)₂⁺] when 3.0 x 10⁻³ moles of Fe(NO₃)₃ and 1.5 x 10⁻³ moles of NaSCN are mixed in a 250 mL solution. The solution shows that the concentration of Fe(SCN)₂⁺ is 1.2 x 10⁻³ M at equilibrium.

asked Jan 23 in Chemical equilibrium by GeorginaThur (370 points)

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1 answer 53 views

Calculate the equilibrium constant (K) for the electrochemical reaction: Mg(s) + 2 Ag+(aq) → Mg2+(aq) + 2 Ag(s) Given that the standard reduction potentials for Ag+ and Mg2+ are +0.80 V and -2.37 V, respectively. The concentration of Ag+ is 0.020 M and the concentration of Mg2+ is 0.080 M.

asked Jan 23 in ElectroChemistry by MarshaReiss (430 points)

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1 answer 52 views

Calculate the equilibrium constant (K$\textsubscript{a}$) for the reaction of acetic acid in aqueous solution if the pH of the solution is 4.76 and the concentration of acetic acid is 0.1 M.

asked Jan 23 in Chemical equilibrium by VioletteErwi (690 points)

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1 answer 50 views

Calculate the equilibrium concentrations of reactants and products for the following reaction at a temperature of 25°C and a pressure of 1 atm:2 NO(g) + Br2(g) ⇌ 2 NOBr(g)Given the initial concentrations are [NO] = 0.20 M, [Br2] = 0.35 M, and [NOBr] = 0.015 M. The equilibrium constant (Kc) for the reaction is 4.8 x 10^2 at 25°C.

asked Jan 23 in Chemical equilibrium by Nydia78K370 (530 points)

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1 answer 40 views

Calculate the equilibrium concentration of each species (in mol/L) in a system containing 0.200 M KI and 0.200 M Cl2 that forms KCl and I2 at equilibrium, given that the equilibrium constant (Kc) is 9.0 x 10^-2 at a certain temperature.

asked Jan 23 in Chemical equilibrium by NQOAnton0782 (530 points)

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1 answer 57 views

Calculate the entropy change when one mole of helium gas is compressed isothermally at 298 K from a volume of 10 L to 2 L. The heat capacity of helium at constant pressure, Cₚ, is 20.8 J/mol*K.

asked Jan 23 in Physical Chemistry by TreyVanhorn (570 points)

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1 answer 7 views

Calculate the entropy change of the following reaction at 25°C and 1 atm pressure:2NH3(g) + 3Cl2(g) → N2(g) + 6HCl(g)Given the standard entropy values are:ΔS°NH3 = 192.5 J/K•molΔS°Cl2 = 223.1 J/K•molΔS°N2 = 191.6 J/K•molΔS°HCl = 186.9 J/K•mol

asked Jan 23 in Chemical thermodynamics by LenardFry234 (570 points)

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1 answer 44 views

Calculate the entropy change of an ideal monatomic gas at 1 atm and 300 K when it expands isothermally to 5 times its initial volume.

asked Jan 23 in Physical Chemistry by JaniceOliver (730 points)

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1 answer 54 views

Calculate the entropy change for the reaction: 2H2(g) + O2(g) → 2H2O(g)given that the standard molar entropies of H2(g), O2(g), and H2O(g) are 130.7 J/mol.K, 205.0 J/mol.K, and 188.8 J/mol.K, respectively.

asked Jan 23 in Chemical thermodynamics by Ines7852940 (490 points)

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1 answer 55 views

Calculate the entropy change for the reaction of 2 moles of methane gas reacting with 4 moles of oxygen gas to form carbon dioxide gas and water vapor at a constant temperature of 298 K. The reaction is balanced and the standard entropy values for methane, oxygen, carbon dioxide, and water vapor are given as -0.242, 205.16, 213.74, and 188.72 J/K/mol, respectively.

asked Jan 23 in Chemical thermodynamics by LukeBqa42900 (550 points)

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1 answer 44 views

Calculate the entropy change for the following chemical reaction at 25 °C: 2H2(g) + O2(g) → 2H2O(l) Given that the standard molar entropy of H2(g), O2(g), and H2O(l) are 130.68 J/mol·K, 205.03 J/mol·K and 70.01 J/mol·K respectively.

asked Jan 23 in Chemical thermodynamics by ChristinaPae (590 points)

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1 answer 55 views

Calculate the entropy change for the combustion of methane at a constant temperature and pressure of 298 K and 1 atm, respectively. The balanced equation for the reaction is:CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)

asked Jan 23 in Chemical thermodynamics by LindaTedesch (450 points)

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