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Recent questions in Chemistry
0
votes
1
answer
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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
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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
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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)
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