Question

experiment to verify the law of conservation of mass in a chemical reaction

Answer 1

Explanation:

Compare the initial mass of the

reaction mixture with the final mass

of the reaction. If the two masses are same with the reasonable limits then the law of conservation of mass stands verified.

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Answer 2

${\huge\bold\pink {E}\bold\blue {x} \bold\purple {p} \bold\green{r} \bold\red {i} \bold\orange {m}\bold\pink {e}\bold\blue {n} \bold\purple {t}}$

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$\huge\sf\red{Objective}$

To verify the law of conservation of mass in a chemical reaction.

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$\huge\sf\red{Materials\: required}$

• $\sf{(i)\: Barium\: chloride\:(BaCl_2•2H_2O)}$
• $\sf{(ii)\: Sodium\: sulphate\:(Na_2SO_4•10H_2O)}$
• $\sf{(iii)\: Distilled\:water}$
• $\sf{(iv)\:Two\:beakers\:(150\:mL)}$
• $\sf{(v)\: One\: beaker\:(250\:mL)}$
• $\sf{(vi)\: Physical\: balance}$
• $\sf{(vii)\: Spring\:balance\:(0-500\:g}$
• $\sf{(viii)\: Polythene\:bag}$
• $\sf{(ix)\:Two\:watch\: glasses\:of\:known\:masses}$
• $\sf{(x)\:Glass\:stirrer }$

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$\huge\sf\red{Theory}$

Law of conservation of mass states that the mass remains conserved during a chemical reaction. In this experiment we shall verify the law of conservation of mass using a precipitation reaction. This reaction is considered as the simplest method to verify this law.

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$\huge\sf\red{Procedure}$

1. Pour 100 mL distilled water in two beakers (150 mL).
2. Using the physical balance and a watch glass of known mass, weigh 7.2 g of $\sf{BaCl_2•2H_2O}$ and dissolve it in a beaker (150 mL) containing 100 mL distilled water.
3. Similarly, weigh 16.1 g of $\sf{Na_2SO_4•10H_2O}$ in another watch glass of known mass and dissolve it in another beaker (150 mL) containing 100 mL distilled water.
4. Take the third beaker (250 mL) and weigh it using a spring balance and polythene bag
5. Mix both solutions of 150 mL beakers in the third beaker (250 mL). Mix the contents using a glass stirrer.
6. On mixing white precipitate of $\sf{BaSO_4}$, appears due to precipitation reaction.
7. Weigh the beaker containing the reaction mixture again to determine the mass of teh precipitation reaction products.
8. Compare the masses of before and after the chemical reaction.

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$\huge\sf\red{Observation}$

Mass of 50 mL distilled water (assuming density as 1g /cc) = 50.0 g

Mass of $\sf{ BaCl_2•H_2O}$ = 3.6 g

Mass of $\sf{BaCl_2}$ solution = 53.6 g

Mass of $\sf{Na_2S_O4•10H_2O}$ = 8.05 g

Mass of $\sf{Na_2SO_4}$ solution =58.05 g

Total mass of reactants (solutions of $\sf{BaCl_2}$ and $\sf{Na_2SO_4)}$ = 53.6 + 58.05 = 111.65 g

Mass of empty 150 mL beaker,m1 =………………….g

Mass of reaction mixture before precipitation, $\sf{m_2= m_1+ 111.65}$ g = ……………………g

Final mass of reaction mixture after precipitation, $\sf{m_3}$ =……………………. g

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$\huge\sf\red{Result}$

1. On comparing the mass of reactants $\sf{(m_2)}$ with the mass of products $\sf{(m_3),}$ we find $\sf{m_2}$ equals $\sf{m_3}$(within reasonable limits).
2. This proves the law of conservation of mass.

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$\huge\sf\red{Precautions}$

1. Accurate measurement of masses should be ensured.
2. The spring balance should be held vertical while taking measurements.
3. Before taking reading, ensure the pointer of the spring balance is at zero mark.
4. The reading of spring balance should be noted when its pointer comes to rest.
5. Use small amount of chemicals.
6. Mix solutions of $\sf{BaCl_2}$ and $\sf{Na_2SO_4}$ slowly with constant stirring.