Answer:
27.70 is 
for the reaction.
Explanation:
The equilibrium constant of the reaction = 
The expression of equilibrium constant is given by :
![K_c=\frac{[CO][Br_2]}{[COBr_2]}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B%5BCO%5D%5BBr_2%5D%7D%7B%5BCOBr_2%5D%7D)
..[1]
The equilibrium constant expression for above reaction can be written as:
![K_c'=\frac{[COBr_2]^2}{[CO]^2[Br]^2}](https://tex.z-dn.net/?f=K_c%27%3D%5Cfrac%7B%5BCOBr_2%5D%5E2%7D%7B%5BCO%5D%5E2%5BBr%5D%5E2%7D)
( from [1])
27.70 is for the reaction.
Answer:
Avogadro's Law
Explanation:
The amount of moles is directly proportional to the volume of the gas under constant temperature and pressure. That is the statement of Avogadro's law. The equation is:
V1n2 = V2n1
<em>Where V is volume and n are moles of 1, initial state and 2, final state of the gas</em>
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That means, right option is:
<h3>Avogadro's Law
</h3>
The empirical formula is SCl_2.
The <em>empirical formula</em> (EF) is the simplest whole-number ratio of atoms in a compound.
The ratio of atoms is the same as the ratio of moles.
So, our job is to calculate the <em>molar ratio </em>of S to Cl.
Assume that you have 100 g of sample.
Then it contains 31.14 g S and 68.86 g Cl.
<em>Step</em> 1. Calculate the <em>moles of each element</em>
Moles of S = 31.14 g S × (1 mol S/(32.06 g S) = 0.971 30 mol S
Moles of Cl = 68.86 g Cl × (1 mol Cl/35.45 g Cl) = 1.9425 mol Cl
<em>Step 2</em>. Calculate the <em>molar ratio</em> of each element
Divide each number by the smallest number of moles and round off to an integer
S:Cl = 0.971 30: 1.9425 = 1:1.9998 ≈ 1:2
<em>Step 3</em>: Write the <em>empirical formula</em>
EF = SCl_2
A strong electrolyte is completely ionized. Ex: NaCl --h2o--> Na^+(aq) + Cl^-(aq)
