1.Which is the largest atom in Group 1?
1 answer:
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Answer:
This question is incomplete
Explanation:
This question is incomplete but some general explanation provides a clear answer to what is been asked in the question.
An ionic/electrovalent compound is a compound whose constituent atoms are joined together by ionic bond. Ionic bond is a bond involving the transfer of valence electron(s) from an atom (to form a positively charged cation) to another atom (to form a negatively charged anion). The atom transferring is usually a metal while the atom receiving is usually a non-metal.
For example (as shown in the attachment), in the formation of NaCl salt, the sodium (Na) transfers the single electron (valence) on it's outermost shell to chlorine (Cl) which ordinarily has 7 electrons on it's outermost shell but becomes 8 after receiving the valence electron from sodium. It should also be noted that Na is a metal while Cl is a non-metal.
The question is incomplete, here is the complete question:
Phosgene, , gained notoriety as a chemical weapon in World War I. Phosgene is produced by the reaction of carbon monoxide with chlorine:
The value of for this reaction is 5.79 at 570 K. What are the equilibrium partial pressures of the three gases if a reaction vessel initially contains a mixture of the reactants in which
and
?
<u>Answer:</u> The equilibrium partial pressure of CO, is 0.257 atm, 0.257 atm and 0.008 atm respectively.
<u>Explanation:</u>
The relation of is given by:
= Equilibrium constant in terms of partial pressure
= Equilibrium constant in terms of concentration = 5.79
= Difference between gaseous moles on product side and reactant side =
R = Gas constant =
T = Temperature = 570 K
Putting values in above equation, we get:
We are given:
Initial partial pressure of CO = 0.265 atm
Initial partial pressure of chlorine gas = 0.265 atm
Initial partial pressure of phosgene = 0.00 atm
The given chemical equation follows:
<u>Initial:</u> 0.265 0.265
<u>At eqllm:</u> 0.265-x 0.265-x x
The expression of for above equation follows:
Putting values in above equation, we get:
Neglecting the value of x = 8.59 because equilibrium partial pressure cannot be greater than initial pressure
So, the equilibrium partial pressure of CO =
The equilibrium partial pressure of
The equilibrium partial pressure of
Hence, the equilibrium partial pressure of CO, is 0.257 atm, 0.257 atm and 0.008 atm respectively.