Recent questions in Chemical equilibrium

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1 answer 70 views

A chemistry student needs to determine the effect of adding NaCl to a solution containing AgNO3 at equilibrium. The original solution had concentration [Ag+]=0.01M and [NO3-]=0.01M, and Ksp=1.8x10^-10. How much NaCl (in grams) is needed to be added to the solution in order to decrease the [Ag+] concentration by a factor of 10?

asked Jan 22 in Chemical equilibrium by DieterSchrod (1.9k points)

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1 answer 105 views

A chemistry student needs to determine the effect of adding more reactant or product on the equilibrium position of the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g)If the student adds more N2 or NH3 to the reaction mixture, how will the equilibrium position change? and how will the equilibrium constant (Kc) for the reaction be affected?

asked Jan 22 in Chemical equilibrium by JeanetteOffi (1.7k points)

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1 answer 94 views

A chemistry student needs to determine how the equilibrium constant (Kc) will change when the volume of the container is increased by a factor of 3 for the following reaction at a certain temperature:2NO2(g) ⇌ N2O4(g)

asked Jan 22 in Chemical equilibrium by Georgianna69 (2.2k points)

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1 answer 105 views

A chemistry student needs to calculate the new value of the ionization constant (Ka) of a weak acid when the temperature is raised from 25°C to 45°C, given that the initial value of Ka is 1.8 x 10^-5 at 25°C and the enthalpy of ionization (ΔHion) is 50.2 kJ/mol.

asked Jan 22 in Chemical equilibrium by DarylBottoml (2.0k points)

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1 answer 114 views

A chemistry student needs to calculate the equilibrium constant (Kc) for the reaction below at a certain temperature: N2(g) + 3H2(g) ⇌ 2NH3(g)Given the initial concentrations of N2, H2, and NH3 are 0.25 M, 0.1 M, and 0.1 M respectively, what is the value of Kc for this reaction at the given temperature?

asked Jan 22 in Chemical equilibrium by LeeAlder0448 (1.5k points)

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1 answer 105 views

A Chemistry student is trying to determine the effect of changing the volume on the equilibrium position of a chemical reaction at constant temperature. If the reaction is initially in equilibrium in a 1 L container with a concentration of [X] = 0.10 M and [Y] = 0.20 M, and then the volume is decreased to 0.4 L, what will be the new equilibrium concentrations of X and Y at the new volume?

asked Jan 22 in Chemical equilibrium by AshleighTheo (1.8k points)

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1 answer 98 views

A chemist mixes 0.1 mol of hydrogen (H2) with 0.2 mol of nitrogen (N2) in a 2 L flask at 400°C. The reaction H2(g) + N2(g) ⇌ 2NH3(g) establishes equilibrium. Calculate the equilibrium concentrations of hydrogen, nitrogen, and ammonia if the Kc value of the reaction at this temperature is 1.5 x 10^-2.

asked Jan 22 in Chemical equilibrium by CarmaC633252 (1.7k points)

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1 answer 91 views

A chemical reaction of N2O4(g) ⇌ 2NO2(g) is established in a closed vessel at a certain temperature. The initial concentration of N2O4 is 0.1M. At equilibrium, the concentration of NO2 is found to be 0.6M. Calculate the equilibrium concentration of N2O4.

asked Jan 22 in Chemical equilibrium by RebekahH3016 (1.9k points)

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1 answer 98 views

A 2.5 L container was initially filled with 0.1 M solution of nitrogen dioxide which decomposes into nitrogen monoxide and oxygen gas according to the following reaction:2NO2(g) ⇌ 2NO(g) + O2(g)After the system has reached equilibrium, the concentration of nitrogen monoxide is found to be 0.05 M. What is the equilibrium concentration of oxygen gas in the container?

asked Jan 22 in Chemical equilibrium by DarylBottoml (2.0k points)

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1 answer 85 views

A 0.50 L vessel contains 1.0 mol of N2(g) and 3.0 mol of H2(g) at equilibrium at 400 K according to the following equation:N2(g) + 3H2(g) ⇌ 2NH3(g)If the volume of the vessel is suddenly decreased to 0.25 L, what will happen to the equilibrium position? Will the concentration of NH3 increase or decrease? Calculate the new equilibrium constant at this new volume.

asked Jan 22 in Chemical equilibrium by SvenJonathan (1.9k points)

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1 answer 94 views

A 0.25 mol/L solution of ethanoic acid (CH3COOH) is mixed with a 0.40 mol/L solution of sodium acetate (CH3COONa). The equilibrium constant for the reaction CH3COOH + NaCH3COO ⇌ CH3COONa + H2O is 1.8 x 10^-5. What is the concentration of CH3COONa at equilibrium?

asked Jan 22 in Chemical equilibrium by MacDeLoitte (1.8k points)

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1 answer 93 views

A 0.1 M solution of ammonia (NH3) has a pH of 11.64 at room temperature. If sodium hydroxide (NaOH) is added to this solution such that the concentration of OH- ions becomes 0.01 M, what will be the new pH of the solution? (Assume that the dissociation of water can be ignored)

asked Jan 22 in Chemical equilibrium by ElvaL9406057 (2.3k points)

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1 answer 84 views

How would adding more reactants to a reaction at equilibrium affect the direction of the reaction and the equilibrium position, and what would be the quantitative effect on the equilibrium constant?

asked Jan 22 in Chemical equilibrium by JanF74978399 (1.6k points)

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1 answer 172 views

A 2.5 L container was initially filled with 0.1 M solution of nitrogen dioxide which decomposes into nitrogen monoxide and oxygen gas according to the following reaction:2NO2(g) ⇌ 2NO(g) + O2(g)After the system has reached equilibrium, the concentration of nitrogen monoxide is found to be 0.05 M. What is the equilibrium concentration of oxygen gas in the container?

asked Jan 22 in Chemical equilibrium by JamaalEnnor6 (1.9k points)

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1 answer 79 views

A 0.50 L vessel contains 1.0 mol of N2(g) and 3.0 mol of H2(g) at equilibrium at 400 K according to the following equation:N2(g) + 3H2(g) ⇌ 2NH3(g)If the volume of the vessel is suddenly decreased to 0.25 L, what will happen to the equilibrium position? Will the concentration of NH3 increase or decrease? Calculate the new equilibrium constant at this new volume.

asked Jan 22 in Chemical equilibrium by Rosaline02Y (2.0k points)

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1 answer 88 views

A 0.25 mol/L solution of ethanoic acid (CH3COOH) is mixed with a 0.40 mol/L solution of sodium acetate (CH3COONa). The equilibrium constant for the reaction CH3COOH + NaCH3COO ⇌ CH3COONa + H2O is 1.8 x 10^-5. What is the concentration of CH3COONa at equilibrium?

asked Jan 22 in Chemical equilibrium by RoderickKyle (2.4k points)

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1 answer 80 views

A 0.1 M solution of ammonia (NH3) has a pH of 11.64 at room temperature. If sodium hydroxide (NaOH) is added to this solution such that the concentration of OH- ions becomes 0.01 M, what will be the new pH of the solution? (Assume that the dissociation of water can be ignored)

asked Jan 22 in Chemical equilibrium by RosarioUsher (2.0k points)

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1 answer 97 views

How would adding more reactants to a reaction at equilibrium affect the direction of the reaction and the equilibrium position, and what would be the quantitative effect on the equilibrium constant?

asked Jan 22 in Chemical equilibrium by DUPMathias4 (2.1k points)

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