Q.2.19 P State the mass law(s) demonstrat... [FREE SOLUTION]

Chapter 2: Q.2.19 P (page 81)

State the mass law(s) demonstrated by the following experimental results, and explain your reasoning:
Experiment 1: A student heats 1.27 g of copper and 3.50 g of iodine to produce 3.81 g of a white compound; 0.96 g of iodine remains.
Experiment 2: A second student heats 2.55 g of copper and 3.50 g of iodine to form 5.25 g of a white compound, and 0.80 g of copper remains.

Short Answer

Expert verified

Individually both experiment 1 and experiment 2 demonstrate the 鈥淟aw of Conservation of Mass鈥� while collectively they demonstrate the 鈥淟aw of Definite Composition.鈥�

Step by step solution

Explanation of Experiment 1

Experiment 1 is given as:

$C o o p e r + I o d i n e = W h i t e c o m p o u n d + I o d i i n e r e m a i n s 1.27 g 3.50 g 3.81 g 0.96 g$

From the equation, we can say that,

$M a s s o f R e a c t a n t (4.77 g) = M a s s o f p r o d u c t s (4.77 g)$

As remains constant before and after the reaction hence it demonstrates the 鈥渓aw of Conservation of Mass.鈥�

Step 2: Explanation of Experiment 2

Experiment 2 is given as:

$C o p p e r + I o d i n e = w h i t e C o m p o u n d + C o p p e r r e m a i n s 2.55 g 3.50 g 5.25 g 0.80 g$

From the equation, we can say that,

$M a s s o f r e a c t a n t (6.05 g) = m a s s o f p r o d u c t s (5.25 g + 0.80 g = 6.05 g)$

As remains constant before and after the reaction hence it demonstrates the 鈥渓aw of Conservation of Mass.鈥�

Both Experiments

Both experiments collectively demonstrate the Law of Definite Composition. The ratio of the reactants reacted the same in both experiments.

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Short Answer

Step by step solution

Explanation of Experiment 1

Step 2: Explanation of Experiment 2

Both Experiments

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