Question

20g of silver nitrate is added to 20g of sodium chloride solution. What change in mass will you expect after the reaction and why?

Answer 1

Complete Question:

20 g silver nitrate solution is added to 20 g of sodium chloride solution. What changes in mass do you expect after the reaction and why? In a given sample of ammonia, 9 g hydrogen and 42 g nitrogen are present. In another sample 5 g hydrogen is present. Calculate the amount of nitrogen in second sample.

Solution:

Balanced Equation,

$\sf{AgNO_{3}+NaCl\longrightarrow AgCl+NaNO_{3}}$

=> Total mass of the reactants = 20g + 20g =40 g

Now, According to the Law of Conservation of Mass, this states that "mass can neither be created nor destroyed, it can only be transformed from one form to another".

For any chemical change total mass of active reactant are always equal to be mass of product formed.

Atoms can neither be created nor be destroyed in a chemical reaction. So, atoms are conserved in a chemical reaction. Therefore, mass of atoms are also conserved in reaction.

So, Mass before reaction = Mass of after reaction

$\sf{\implies \dfrac{Mass\;of\;Nitrogen\;in\;sample\;1}{Mass\;of\;Hydrogen\;in\;sample\;1} = \dfrac{Mass\;of\;Nitrogen\;in\;sample\;2}{Mass\;of\;Hydrogen\;in\;sample\;2}}$

$\sf{\implies \dfrac{42}{9}=\dfrac{x}{5}}$

$\sf{\implies x = \dfrac{45\times 5}{9}}$

$\large{\boxed{\boxed{\blue{\sf{\implies x = 23.33\;g}}}}}$

Answer 2

Answer:

answer

Explanation:

20g of silver nitrate is added to 20g of sodium chloride solution. What change in mass will you expect after the reaction and why?