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Multiple choice chemistry p- block elements-ii compounds of phosphorus - pcl3 phosphorus halides compounds of phosphorus compounds of phosphorus- pcl5

Is ${PCl} _{3}$ soluble in water?

  1. Not Soluble

  2. May be

  3. Partially soluble

  4. Soluble
Reveal answer Fill a bubble to check yourself
D Correct answer
Explanation
like dissolve like. It means polar molecules dissolves in polar molecules and non-polar molecules.Molecules dissolves in non polar molecules $Water$ and $PCl _3$ both are polar molecules because of their shape and electronegative difference between $H$ and $O$ in water and $P$ and $Cl$ in $PCl _3$. Hence $PCl _3$ is solube in water.
$PCl _3$ dissolve in water to form phosphorous acid.
$PCl _3$ $+$ $3H _2O$  $\longrightarrow $   $H _3PO _3$ $+$ $3HCl$
Multiple choice chemistry p- block elements-ii compounds of phosphorus - pcl3 phosphorus halides compounds of phosphorus compounds of phosphorus- pcl5

How is $ {P}{Cl} _{3} $ produced industrially?

  1. Reacting chlorine with white phosphorus

  2. Reacting chlorine with phosphorus acid

  3. Reacting chlorine with black phophorous

  4. All of the above
Reveal answer Fill a bubble to check yourself
A Correct answer
Explanation
Industrially Phosphorous trichloride is prepared by the reaction of Chlorine with a solution of white Phosphorous in phosphorous trichloride.
The reaction is given by:
$P _4$ $+$ $6Cl _2$ $\longrightarrow $ $4PCl _3$
Multiple choice chemistry p- block elements-ii compounds of phosphorus - pcl3 phosphorus halides compounds of phosphorus compounds of phosphorus- pcl5

What is the physical state of ${PCl} _{3}$ under normal condition?

  1. Solid

  2. Liquid

  3. Gaseous

  4. None of these
Reveal answer Fill a bubble to check yourself
B Correct answer
Explanation

${PCl} _{3}$ is liquid under normal conditions. ${PCl} _{3}$ is a covalent compound. Phosphorus and each of the chlorine atoms fulfil their octet by mutually sharing their valence electrons. In general, covalent compounds have weak bond energy and hence they form liquid.

Multiple choice chemistry introduction to analytical chemistry interpreting a balanced chemical reaction percentage yield stoichiometric calculations

$1.25$ g of sample of limestone on heating gives $0.44$ g carbon dioxide. The percentage purity of $CaCO _3$ in limestone is:

  1. $75\%$
  2. $85\%$
  3. $90\%$
  4. $80\%$
Reveal answer Fill a bubble to check yourself
D Correct answer
Explanation

$CaCO _3$ $\quad \underrightarrow \Delta\quad  CaO +CO _2$

Moles of $CO _2$ produced =$\cfrac{0.44}{44}$$=0.01$ moles
Moles of pure $CaCO$$ _3$ required $=0.01$ moles
$=0.01 \times 100g$
$=1g$
Therefore $\%$ purity of $CaCO$$ _3$  in limestone =$\cfrac{1}{1.25}\times 100$
$=80\%$