Law of Constant Proportions

Q. 1.375 g of cupric oxide was reduced by heating in a current of hydrogen and the mass of copper that remained was 1.098 g . In another experiment 1.179 g copper was dissolved in nitric acid and the resulting copper nitrate was converted into cupric oxide . The mass of cupric oxide formed was 1.476 g . Show that these results illustrate the law of constant composition.

Q. Hydrogen and oxygen combine in the ratio of 1:8 by mass to form water.what mass of oxygen gas would be required to react completely with 3g of hydrogen

Q.

Give two drawbacks of Daltons atomic theory of matter.

Q.

State law of reciprocal proportion with an example.

Q.

What Are the Assumptions of Law of Variable Proportions?

Q.

Copper oxide was prepared by 2 different methods. In case 1, 1.75 g of metal gives 2.19 grams of oxide. In case 2, 1.14 grams of metal gives 1.43 grams of oxide. How we can illustrate this according to the law of constant proportion

Q.

1gram alloy of aluminium and magnesium reacted with hcl and formed agcl3 mgcl2 and evolved hydrogen gas . H2 was contained in a container with volume 1200ml at 0 centigrade . Find the composition of aluminium and magnesium in the alloy

Q.

A hydrated salt, Na₂SO_4^. nH₂O undergoes 56% loss in weight on heating and become anhydrous. The value of n(approximately) will be :

(PLEASE ANSWER IN A EASY TO UNDERSTAND MANNER)

Q.

When 3.0 g of carbon is burnt in 8.00 g oxygen, 11.00 g of carbon dioxide is produced. What mass of carbon dioxide will be formed when 3.00 g of carbon is burnt in 50.00 g of oxygen? Which law of chemical combinations will govern your answer?

Q.

The molecular formula of water is H₂O.

Write the information do you get from this formula

Q.

What is the equivalent mass of ${\mathrm{CH}}_3\mathrm{COOH}$?

Q.

Calculate the mass of $1\times {10}^{23}$ molecules of methane.

Q.

2 oxides of a certain metal was separately heated in a current of hydrogen until constant weights were obtained. The water produced in each case was carefully collected and weighed. 2 grams of each oxide gave respectively 0.2517 grams and 0.4526 grams of water. Show that these results establish the law of multiple proportion.

Q.

Which law is also known as Law of constant composition?

Q.

A sample of Ammonia molecule irrespective of source contains 82.35% of nitrogen and 17.65% of hydrogen by mass obeys:

1. Avogadros law

2. Law of conservation of mass

3. Law of multiple proportion

4. Law of definite proportion

Q.

What is the ratio of carbon and oxygen in carbon dioxide?

Q. Magnesium and oxygen combine in the ratio of 3 : 2 by mass to form magnesium oxide. What mass of oxygen gas would be required to react completely with 24 g of magnesium ?

Q. Who proposed the law of constant proportions?

1. Joseph Proust
2. Antoine Lavoisier
3. John Dalton
4. Ernest Rutherford

Q.

What is the mass ratio of nitrogen to hydrogen in an NH₃ molecule?

1. 8:1

2. 3:14

3. 14:3

4. 1:8

Q. A chemical compound always contains the elements combined in fixed proportion by mass.

1. True
2. False

Q.

State the difference between Atomic mass and molecular mass?

Find the molecular mass of HNO3.

Q.

What is a compound? Give an example.

Q.

The mass ratio of carbon to hydrogen in methane is 3:1. How much amount of hydrogen is required to react with 36 g of carbon to form methane?

1. 10 g

2. 12 g

3. 16 g

4. 30 g

Q.

In hydrogen peroxide $\left(H_2{O}_2\right)$, the proportion of hydrogen by mass is :

1. 1 : 16

2. 8 : 1

3. 16 : 1

Q.

Can you give me all formulas of atoms and molecules as it will help me as exams are approaching?

Q.

To account for the atomic mass of nitrogen as $14.0067$ what should be the ratio of ${}^{15}\mathrm{N}$ and ${}^{14}\mathrm{N}$ atoms in natural nitrogen?

Q. Assertion: Isotopes are electrically neutral
Reason: Isotopes are species with same mass number but different atomic number

1. Both Assertion and Reason are correct and Reason is the correct explanation of Assertion
2. Both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion
   
3. Assertion is incorrect but Reason is correct
4. Assertion is correct but Reason is incorrect

Q.

In water, the proportion of oxygen and hydrogen by mass is :

1. 1 : 8

2. 1 : 4

3. 4 : 1

4. 8 : 1

Q. Question 2
When 3.0 g of carbon is burnt in 8.00 g oxygen, 11.00 g of carbon dioxide is produced. What mass of carbon dioxide will be formed when 3.00 g of carbon is burnt in 50.00 g of oxygen? Which law of chemical combinations will govern your answer?

Q.

Calculate the number of moles in 48 g of oxygen atoms.