Answer:
3.9
Explanation:
Let's consider the following reaction at equilibrium.
CO(g) + Cl₂(g) ↔ COCl₂(g)
We can find the pressures at equilibrium using an ICE chart.
CO(g) + Cl₂(g) ↔ COCl₂(g)
I 0.96 1.15 0
C -x -x +x
E 0.96-x 1.15-x x
The sum of the partial pressures is equal to the total pressure.
pCO + pCl₂ + pCOCl₂ = 1.47
(0.96-x) + (1.15-x) + x = 1.47
2.11 - x = 1.47
x = 0.64
The pressures at equilibrium are:
pCO = 0.96 - x = 0.32 atm
pCl₂ = 1.15 - x = 0.51 atm
pCOCl₂ = x = 0.64 atm
The pressure equilibrium constant (Kp) is:
Kp = pCOCl₂ / pCO × pCl₂
Kp = 0.64 / 0.32 × 0.51
Kp = 3.9
The temperature increase when energy in is greater than energy out, and temperature decreases when energy out is than energy in.
Definition of a compound
A substance made up of atoms from two or more elements that are chemically bonded together
Initiation <span>occurs when mRNA, tRNA, and an amino acid meet up inside the ribosome. </span>Elongation occurs when amino acids are continually added to the line, forming a long chain bound together by peptide bonds.
Answer:
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