N2 (g)+ 3 H2 (g)↔ 2 NH3 (g) Explain what would happen to the above equilibrium...

N_{2 (g)}+ 3 H_{2 (g)}↔ 2 NH_3
(g)

Explain what would happen to the above equilibrium equation if ...

ammonia gas (NH₃) was removed from the system?

more hydrogen gas (H₂) was added to the system?

volume was decreased?

nonreactive argon gas (Ar) was added to the system?

A mixture of hydrogen gas and iodine is allowed to react in a reaction vessel. Once equilibrium is established, the equilibrium concentrations are found to be [H₂]=0.48 mol/L, [I₂]=0.33 mol/L, and [HI]=3.11 mol/L. Calculate the value of Keq and determine if this equilibrium favors the products or reactants.

Expert Solution

queen_honey_blossom answered 2 years ago

1) Consider the equilibrium reaction N2(g) + 3 H2(g) ↔ 2 NH3(g) + 91.8 kJ Using...

1) Consider the equilibrium reaction N2(g) + 3 H2(g) ↔ 2 NH3(g) + 91.8 kJ Using Le Chatelier’s Principle, Name two specific ways this equilibrium can be shifted to the right to increase production of NH3. 2) In the reaction below, NH3(g) + H2O(l) ↔ NH2 - + H3O + The equilibrium constant is 1 x 10 -34. Is this reaction likely to take place? Explain your answer.

For the reaction N2(g) + 3 H2(g) equilibrium reaction arrow 2 NH3(g) at 25.0°C, the Kc...

For the reaction N2(g) + 3 H2(g) equilibrium reaction arrow 2 NH3(g) at 25.0°C, the Kc of the reaction is 5.4 ✕ 105 and the ΔG° is −32.7 kJ/mol. Use the given concentrations to determine the following. [N2] = 0.0027 M [H2] = 0.0045 M [NH3] = 0.20 M (a) Determine the ΔG of the reaction. (b) Determine which direction the reaction will proceed in order to reach equilibrium.

Consider the reaction: 3 H2 (g) + N2 (g) ⇋ 2 NH3 (g) In a given...

Consider the reaction: 3 H2 (g) + N2 (g) ⇋ 2 NH3 (g) In a given reaction, the initial concentrations of reactants and product are: [H2] = 0.150 M; [N2] = 0.300 M ; [NH3] = 0.000 M If the equilibrium concentration of H2 is 0.0900 M, what is Kc for the reaction under these conditions?

At 400 K, the reaction N2 (g) + 3 H2 (g) → 2 NH3 (g) reaches...

At 400 K, the reaction N2 (g) + 3 H2 (g) → 2 NH3 (g) reaches equilibrium when the partial pressures of nitrogen, hydrogen, and ammonia gases are 4.00 atm, 1.00 atm, and 1.05 x 10^−2 atm, respectively. (a) Compute the value of the equilibrium constant, KP at 400K. (b) Compute the standard Gibbs free energy of this reaction at 400K. Express the result in kJ/mol. (c) Would the system be at equilibrium at 400 K if the partial pressures...

Consider the reaction, N2(g) + 3 H2(g) → 2 NH3(g). Suppose 56 g of N2(g) reacts...

Consider the reaction, N2(g) + 3 H2(g) → 2 NH3(g). Suppose 56 g of N2(g) reacts with 18 g of H2(g). d. What is the limiting reactant? e. When the reaction is complete, how many grams of NH3(g) are produced? f. When the reaction is complete, how many grams of N2(g) remain? g. When the reaction is complete, how many grams of H2(g) remain? h. If the reaction actually produced 55 g of NH3(g), what is the percent yield?

Consider the reaction 2 NH3 (g) ? N2 (g) + 3 H2 (g). Suppose 6 moles...

Consider the reaction 2 NH3 (g) ? N2 (g) + 3 H2 (g). Suppose 6 moles of pure ammonia are placed in a 1.0 liter flask and allowed to reach equilibrium. If X represents the concentration (in M) of nitrogen present in the system once equilibrium is reached, which of the following will represent the concentration of ammonia in M? Show work A) 6

Given N2 + 3 H2 → 2 NH3 If 5.55 g of each reactant are used,...

Given N2 + 3 H2 → 2 NH3 If 5.55 g of each reactant are used, what is the theoretical mass, in grams, of ammonia that will be produced? Also, what is the percent yield for this reaction if 5.55 g of ammonia are obtained experimentally?

An equilibrium mixture of N2, H2 and NH3 at 700K contains 0.036M H2 and 0.015M H2....

An equilibrium mixture of N2, H2 and NH3 at 700K contains 0.036M H2 and 0.015M H2. At this temperature, Kc for the reation N2(g)+3H2(g) <> 2NH3(g) is 0.29. What is the concentration of NH3?

(a) Write a stoichiometric table for the reaction N2 + 3 H2  2 NH3 for...

(a) Write a stoichiometric table for the reaction N2 + 3 H2  2 NH3 for an isothermal, isobaric flow system with equimolar (or equal molar) feeds of N2 & H2. (b) If the entering total pressure is 16.4 atm and the entering temperature is 1727 oC, calculate the concentration of hydrogen and nitrogen entering the reactor. (c) Plot the gas composition (molar fractions) as a function of the conversion. Is there anything worth noticing? Can you explain it? What...

1.30 g H2 is allowed to react with 10.4 g N2, producing 2.53 g NH3. What...

1.30 g H2 is allowed to react with 10.4 g N2, producing 2.53 g NH3. What is the theoretical yield in grams for this reaction under the given conditions? What is the percent yield for this reaction under the given conditions?

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