Recent questions in Chemistry

0 votes

1 answer 68 views

Calculate the equilibrium constant (Kc) of the chemical reaction: 2NOCl(g) ⇌ 2NO(g) + Cl2(g) where the concentration of NOCl is 0.5 M, NO is 0.2 M, and Cl2 is 0.1 M at equilibrium at a certain temperature.

asked Jan 23 in Chemical reactions by OnitaLoftus1 (2.3k points)

0 votes

1 answer 57 views

Calculate the equilibrium constant (Kc) for the reaction: 2A(g) + B(g) ⇌ C(g) + D(g), if the concentration of A is 0.25 M, the concentration of B is 0.10 M, the concentration of C is 0.30 M and the concentration of D is 0.20 M at equilibrium.

asked Jan 23 in Chemical thermodynamics by ElvaL9406057 (2.3k points)

0 votes

1 answer 78 views

Calculate the equilibrium constant (Kc) for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) if the equilibrium concentration of nitrogen (N2) is 0.025 M, hydrogen (H2) is 0.10 M, and ammonia (NH3) is 0.015 M.

asked Jan 23 in Chemical reactions by DXGMilagros4 (1.9k points)

0 votes

1 answer 70 views

Calculate the equilibrium constant (Kc) for the reaction between nitrogen gas (N2) and hydrogen gas (H2) to form ammonia gas (NH3) at a temperature of 400 K. The reaction is written as follows: N2(g) + 3H2(g) ⇌ 2NH3(g) Given the equilibrium concentrations are [N2] = 0.10 M, [H2] = 0.20 M, and [NH3] = 1.0 M.

asked Jan 23 in Chemical thermodynamics by JeremiahMoli (1.7k points)

0 votes

1 answer 47 views

Calculate the equilibrium constant (Kc) for the reaction between iodine (I2) and potassium iodide (KI) in an aqueous solution, given that at equilibrium, the concentration of iodine is 0.008 M and the concentration of potassium iodide is 0.15 M. The balanced equation for the reaction is given below:I2 (aq) + 2KI (aq) ⇌ 2K+ (aq) + 2I- (aq)

asked Jan 23 in Chemical equilibrium by FawnSharrow (1.9k points)

0 votes

1 answer 62 views

Calculate the equilibrium constant (Kc) for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) if at a certain temperature, the initial concentrations of SO2, O2, and SO3 are 0.1 M, 0.2 M, and 0 M, respectively. The equilibrium concentrations of SO2 and SO3 are both 0.05 M. Assume the reaction takes place in a closed system at constant pressure.

asked Jan 23 in Chemical thermodynamics by OnaSchnell25 (1.8k points)

0 votes

1 answer 63 views

Calculate the equilibrium constant (Kc) for the following reaction at 300 K: N2(g) + 3 H2(g) ↔ 2 NH3(g) given that at equilibrium, the concentration of N2 is 0.12 M, H2 is 0.20 M, and NH3 is 0.16 M.

asked Jan 23 in Chemical equilibrium by Dwain5313275 (2.5k points)

0 votes

1 answer 64 views

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 Cameron54A25 (1.9k points)

0 votes

1 answer 65 views

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 JeroldStonem (1.6k points)

0 votes

1 answer 49 views

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 StuartCarson (2.4k points)

0 votes

1 answer 51 views

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 AhmadEho9450 (1.6k points)

0 votes

1 answer 50 views

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 LibbyHollera (2.4k points)

0 votes

1 answer 59 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 QJXClarice2 (2.5k points)

0 votes

1 answer 59 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 CorneliusU11 (1.7k points)

0 votes

1 answer 64 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 RandellBeggs (2.0k points)

0 votes

1 answer 63 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 JacquelynDos (1.7k points)

0 votes

1 answer 68 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 DaleHaveman (2.1k points)

0 votes

1 answer 63 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 ElidaHaskins (1.7k points)

0 votes

1 answer 54 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 ThaliaSheil (2.0k points)

0 votes

1 answer 48 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 Wilbur29087 (1.8k points)

Categories