For the synthesis of ammonia N2(g) + 3H2(g) = 2NH3(g) the equilibrium constant K, at 375°C is 1.2. Starting with [H2lo = 0.76 M, [N2lo = 0.60 M and [NH310 = 0.48 M, which concentration(s), if any, will have increased when the mixture comes to equilibrium? %3D %3D %3D H2 N2 N2 and H2 NH3 There will be no change
For the synthesis of ammonia N2(g) + 3H2(g) = 2NH3(g) the equilibrium constant K, at 375°C is 1.2. Starting with [H2lo = 0.76 M, [N2lo = 0.60 M and [NH310 = 0.48 M, which concentration(s), if any, will have increased when the mixture comes to equilibrium? %3D %3D %3D H2 N2 N2 and H2 NH3 There will be no change
Chemistry
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![Select the single best answer.
For the synthesis of ammonia
N2(g) + 3H,(g) 2NH3(g)
the equilibrium constant K. at 375°C is 1.2. Starting with [H,lo = 0.76 M, [N2lo = 0.60 M and
[NH3]0
= 0.48 M, which concentration(s), if any, will have increased when the mixture comes to
equilibrium?
H2
N2
N2 and H,
NH3
There will be no change](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd2745bc2-3d98-4823-b805-8980cae50ead%2F8e213e42-b63d-455a-8abd-4ceda6ce1960%2Fylnpccm_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Select the single best answer.
For the synthesis of ammonia
N2(g) + 3H,(g) 2NH3(g)
the equilibrium constant K. at 375°C is 1.2. Starting with [H,lo = 0.76 M, [N2lo = 0.60 M and
[NH3]0
= 0.48 M, which concentration(s), if any, will have increased when the mixture comes to
equilibrium?
H2
N2
N2 and H,
NH3
There will be no change
Expert Solution

Step 1
The equilibrium reaction given is,
=>
Given: Equilibrium constant, Kc = 1.2
Initial concentration of H2 = 0.76 M
Intiial concentration of N2 = 0.60 M
And initial concentration of NH3 = 0.48 M
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