The balanced chemical equation is given as

C + O₂ CO₂

Given mass of CO₂ = 220mg = 0.22g

44g of CO₂ is produced from 6.022 x 10²³ oxygen molecules.

0.22g of CO₂ can be produced from 3.011 x 10²¹ oxygen molecules.

The balanced chemical equation is given as:

S + O₂ SO₂

According to the reaction

6.022 x 10²³ molecules of SO₂ are produced from 32g sulphur.

6.022 x 10²⁴ molecules of SO₂ are produced from = 320g sulphur

Similarly,

6.022 x 10²³ molecules of SO₂ are produced from 32g of oxygen

6.022 x 10²⁴ molecules of SO₂ can be produced from = 320g oxygen

Two atoms of Carbon:

1 mole of carbon = 12g
1 mole of carbon = 6.022 x 10²³ carbon atom

Thus,
6.022 x 10²³ carbon atom has mass 12g
2 carbon atom has mass = 3.98 x 10^-23 g carbon.

Three molecules of hydrogen:

1 mole of hydrogen molecule = 2g
1 mole of hydrogen molecule = 6.022 x 10²³ hydrogen molecule

Thus,
6.022 x 10²³ hydrogen molecule has mass 2g hydrogen.

3 hydrogen molecules has mass = 9.96 x 10^-24g

Given,

The given weight of CO = 0.28 g
The molecular weight of CO = 28g

No. of moles of CO = 0.01 mole

We know that,

1 mole of CO contains 6.022 x 10²³ molecules
0.01 mole of CO contains 0.01 x 6.022 x 10²³ molecules = 6.022 x 10²¹ molecules

The number of molecules left is (6.022 x 10²¹ - 2 x 10²¹) = 4.022 x 10²¹ molecules

We know that,

6.022 x 10²³ molecules of CO = 1 mole of CO

4.012 x 10²¹ molecules of CO = 6.68 x 10^-3

Hence, no. of mole of CO left is 6.68 x 10^-3

Given,

No. of atoms of an element = 2 x 10²¹
Mass of atoms of an element = 0.4g

According to the questions,

2 x 10²¹ atoms of an element has mass 0.4g
6.022 x 1023 atoms of element has mass = 120.44g

i.e. 1 mole of atom of an element has mass 120.44g

Hence, the mass of 0.5 mole of an elements is 0.5 x 120.44g = 60.22g

In 1803, John Dalton proposed the law of multiple proportion. Law of multiple proportion states that, "When two elements which combine to form two or more different compounds, then the weight of one of the elements which combine with the constant weight of the other bear simple whole number ratio."

The law of conservation of mass is known as indestructibility of matter because there is no loss of mass when reactant reacts to form product i.e. total mass of the reactant is equal to total mass of the product.

C + 2H₂ CH₄

Total weight of reactant = 16g
Total weight of product = 16g
Total weight of reactant = total weight of product

So these data show the law of conservation of mass.

Statement:

Total sum of mass and energy of system remains constant, but they can be interconverted.

When two different elements combine separately with the fixed weight of the elements, the ratio in which they do so will be the same or some simple multiple of the ratio which they combine together.

Under similar condition of temperature and pressure, gaseous reactants and products combine in a simple whole number ratio of their volumes.

According to the Dalton's atomic theory, law of conservation of mass states that, "Matter is made up if extremely small indivisible particles which can neither be created nor be destroyed."

Statement:

A chemical compound always contains the same elements combined together in the fixed ratio by weight, irrespective of the origin.

Law of reciprocal proportion relates the proportions in which elements combine across a number of different elements. It is also called as equivalent proportion.

Example:

If element A combines with element B and also with C, if B and C combine together, the proportion by weight in which they do so will be simply related to the weights of B and C which separately combine with a constant weight of A.

Nitrogen combines with oxygen to form various oxide.

The ratio of different weight of oxygen 24, 40 combining with fixed weight of nitrogen 14 is 24:40 i.e. 3:5 which is simple whole number ratio. The given data illustrate the law of multiple proportions.

Statement:

"When two elements combine to form more than one compound, then the different weight of one element combining with a...

Solution:
Given,
In the compound X,
% of hydrogen = 25% & % of carbon = (100 – 25)% = 75% 25 parts by weight of hydrogen combine with 75 parts by weight of carbon.
1 part by weight of hydrogen combine withparts by weight of carbon
= 3 parts by weight of carbon

In the compound Y,
% of hydrogen = 14.3% & % of carbon = (100 – 14.3)% = 85.7% 14.3 parts by weight of hydrogen combine with 85.7 parts by weight of carbon
1 part by weight of hydrogen combine withparts by weight of carbon
=5.99 parts by...

Here,
In P₂O₃, 62gm of Phosphorous combined with 48gm of oxygen.
In P₂O₅, 62gm of Phosphorous combined with 80gm of oxygen.

Ratio of mass of oxygen in P₂O₃and P₂O₅= 48:80 = 3:5 which is simple whole number ratio.

In this reaction, the ratio of mass of oxygen in PO and PO combined with fixed mass of phosphorous bear simple whole number ratio.

This illustrates, the law of multiple proportion of stoichiometry which states that,"Whentwo elements combined to each other to give two or more productsthen...

Ans:Solution:
Given,
Experiment 1,

Wt. of zinc = 0.936 g
Wt. of oxide = 1.165 g
Wt. of oxygen = (1.165 – 0.936) g = 0.229 g

The ratio of weight of oxygen is to zinc in zinc oxide is

Experiment 2,

Wt. of zinc = 1.236 g
Wt. of oxide = 1.538 g
Wt. of oxygen = (1.538 – 1.236) g = 0.302 g

The ratio of weight of oxygen is to zinc in this oxide is

The ratio of weight of oxygen to weight of zinc in both the oxides is the same. Hence, given data
illustrate the law of definite proportions.

Alternative Method

In...

Ans:
In this reaction, the total mass of reactants is equal to the total mass of the product.

This illustrates the law of conservation of mass which states, "Under similar conditions of temperature and pressure, the total mass of reactants in any chemical reaction is equal to the total mass of product."