Question

In: Chemistry

Consider the chemical equation 2NH3 ? N2 + 3H2. the equilibrium is to be established in...

Consider the chemical equation 2NH3 ? N2 + 3H2. the equilibrium is to be established in a 1 liter container at 1,000 K, where Kc= 4.0*^-2. Initially1,220 moles of NH3 are present. Estimate equilibrium concentration of H2.

Expert Solution

Solution

Given data

Kc =4.0*10^-2

Initial moles of NH3 = 1220

Equilibrium concentration of H2= ?

Lets make the ICE table

2NH3 ------ > N2 + 3H2

I 1220 M 0 0

C -2x +x +3x

E 1220-x x 3x

Lets write the equilibrium constant expression

Kc =[N2][H2]³/[NH3]²

Now lets out the values in the formula

4.0*10^-2 = [x][3x]³/[1220-2x]²

4.0*10^-2 *[1220-2x]²=[x][3x]³

By solving this equation we get

X= 1.16

Therefore the equilibrium concentration of H2 = 3x = 3*1.16 = 3.48 M

queen_honey_blossom answered 11 months ago

I'm trying to under stand the Haber process and this equilibrium reaction N2 +3H2 -----> 2NH3...

I'm trying to under stand the Haber process and this equilibrium reaction N2 +3H2 -----> 2NH3 + energy. In order to increase the yields of ammonia 1. remove amonia as it is formed 2. add an inhibitor 3. heat the reaction vessel 4. decrease the pressure in the reaction vessel.

Consider the following system at equilibrium N2(g)+3H2(g) <------> 2NH3(g)+ heat Indicatre which way the reaction wil...

Consider the following system at equilibrium N2(g)+3H2(g) <------> 2NH3(g)+ heat Indicatre which way the reaction wil shift when making the following changes 1. Decreasing in the temperture 2. Increasing in the temperture 3. Removing some of NH3 4. Removing some of the H2O 5. Adding some O2 6. Removing some N2 ****Pick from these answers **** A. Forward reaction will increase B. Reverse reaction will increase C. There will be no change in either direction

For the reaction: 3H2(g) + N2(g) ↔ 2NH3(g) Kc = 480 At equilibrium, a reaction contains...

For the reaction: 3H2(g) + N2(g) ↔ 2NH3(g) Kc = 480 At equilibrium, a reaction contains 0.3M N2(g) and 4.0M NH3(g). What is the concentration of H2(g)?

Kp for the equilibrium N2(g)+ 3H2(g) <> 2NH3(g) is 4.51 x 10^-5 at 450C. For each...

Kp for the equilibrium N2(g)+ 3H2(g) <> 2NH3(g) is 4.51 x 10^-5 at 450C. For each of the mixtures listed here, indicated whether the mixture is at equilbrium at 450C. If it is not at equilibrium , indicate the direction in which the mixture must shift to achieve equilibrium. a) 98 atm NH3, 45 atm N2, 55atm H2 b) 57 atm NH3 143 atm N2, no H2 c)13 atm NH3, 27 atm N2, 82 atm H2

The Haber reaction for the manufacture of ammonia is: N2 + 3H2 → 2NH3 Without doing...

The Haber reaction for the manufacture of ammonia is: N2 + 3H2 → 2NH3 Without doing any experiments, which of the following can you say MUST be true? The activation energy is positive. Disappearance rate of N2 = 3 (Disappearance rate of H2). Disappearance rate of H2 = 3 (Disappearance rate of N2). The reaction is not an elementary reaction. The reaction is first order in N2. Reaction rate = -Δ[N2]/Δt. Δ[H2]/Δt will have a positive value.

N2 + 3H2>>>2NH3 Using the equation above, calculate how many grams of NH3 you would have...

N2 + 3H2>>>2NH3 Using the equation above, calculate how many grams of NH3 you would have if you started with 2.37 g of N2 and 2.37 g of H2?

The Kc for the following reaction at 225 ∘C is 1.7×102. 3H2(g)+N2(g)⇌2NH3(g) If the equilibrium mixture...

The Kc for the following reaction at 225 ∘C is 1.7×102. 3H2(g)+N2(g)⇌2NH3(g) If the equilibrium mixture contains 0.22 M H2 and 0.017 M N2, what is the molar concentration of NH3? Express your answer to two significant figures and include the appropriate units. Enter your answer using dimensions of chemical concentration.

Ammonia can be synthesized by the reaction: 3H2+N2=>2NH3 What is the theoretical yield of ammonia, in...

Ammonia can be synthesized by the reaction: 3H2+N2=>2NH3 What is the theoretical yield of ammonia, in kilograms, that we can synthesize from 5.35 kg of H2 and 31.8 kg of N2?

Consider the reaction N2(g) + 3H2(g) → 2NH3(g)ΔH o rxn = −92.6 kJ/mol If 2.0 moles...

Consider the reaction N2(g) + 3H2(g) → 2NH3(g)ΔH o rxn = −92.6 kJ/mol If 2.0 moles of N2 react with 6.0 moles of H2 to form NH3, calculate the work done (in joules) against a pressure of 1.0 atm at 25 degrees celsius. What is ΔU for this reaction? Assume the reaction goes to completion.

Ammonia can be synthesized by the reaction: 3H2(g) + N2(g) —-> 2NH3(g) What is the theoretical...

Ammonia can be synthesized by the reaction: 3H2(g) + N2(g) —-> 2NH3(g) What is the theoretical yield of ammonia, in kg, that we can synthesize from 5.43kg of H2 and 32.4 kg of N2?