Similarities and differences between covalent bonds and molecular interactions

1 answer:

3 0

Covalent bonds are formed between atoms which have
- unsatisfied valency 
- no inert gas electronic configuration 
- These are directional bonds 
- formed by sharing of electrons 

Intermolecular forces 
- much weaker than covalent bond 
- These are not directional (except Hydrogen bonds) 
- These are more electrostatic in nature 
- exist between stable molecules 
- can be Hydrogen bonding, dipole-dipole and induced dipole-induced dipole

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What is the limiting reactant and theoretical yield if 0.483 mol of Ti and 0.911 mol Clare used in this reaction: Ti + 2Cl2 → Ti

Mariana [72]

Answer : The limiting reactant is $Cl_2$ and the theoretical yield will be 86.45 grams.

Explanation : Given,

Moles of $Ti$ = 0.483 mole

Moles of $Cl_2$ = 0.911 mole

Molar mass of $TiCl_4$ = 190 g/mole

First we have to calculate the limiting and excess reagent.

The given balanced chemical reaction is,

$Ti+2Cl_2\rightarrow TiCl_4$

From the balanced reaction we conclude that

As, 2 moles of $Cl_2$ react with 1 mole of $Ti$

So, 0.911 moles of $Cl_2$ react with $\frac{0.911}{2}=0.455$ moles of $Ti$

From this we conclude that, $Ti$ is an excess reagent because the given moles are greater than the required moles and $Cl_2$ is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of $TiCl_4$ .

As, 2 moles of $Cl_2$ react to give 1 moles of $TiCl_4$

So, 0.911 moles of $Cl_2$ react to give $\frac{0.911}{2}=0.455$ moles of $TiCl_4$

Now we have to calculate the mass of $TiCl_4$ .

$\text{Mass of }TiCl_4=\text{Moles of }TiCl_4\times \text{Molar mass of }TiCl_4$