Law of definite proportions - class-VIII
Description: law of definite proportions | |
Number of Questions: 61 | |
Created by: Tanuja Atwal | |
Tags: matter : nature and behaviour evs atoms, molecules and chemical reactions the structure of the atom let's play with water chemistry some basic concepts of chemistry quantitative chemistry atoms and molecules basic concepts of chemistry particle nature, basic units stoichiometry measurement of matter |
In an experiment, 2.4 g of iron oxide on reduction with hydrogen gave 1.68 g of iron. In another experiment, 2.9 g of iron oxide gave 2.09 g of iron on reduction. Which law is illustrated from the above data?
A sample of calcium carbonate $(CaCO _{3})$ has the following percentage composition:
Ca = 40%; C = 12%; O = 48%.
If the law of constant proportions is true, then the weight of calcium in 4 g of a sample of calcium carbonate from another source will be:
A sample of calcium carbonate $\left( CaC{O} _3 \right)$ has the following percentage composition:
Ca = 40%; C = 12%; O = 48%.
If the law of constant proportions is true, then the weight of calcium in 4 g of a sample of calcium carbonate from another source will be ?
Different samples of water were found to contain hydrogen and oxygen in the ratio of 1 : 8. This shows the law of:
All samples of carbon dioxide contain carbon and oxygen in the mass ratio of $3 : 8$. This is in agreement with the law of :
Law of constant composition is also called as the law of :
When hydrogen and oxygen combine to form water, they form:
In ammonia, nitrogen and hydrogen always combine in $14:3$ ratio by mass. This is in agreement with :
Law of definite proportion does not apply to nitrogen oxide because:
The ratio of mass of nitrogen and oxygen in nitric oxide is in :
A solution of copper oxide was prepared by heating, igniting and precipitation. Which of the following method will give higher ratio of copper oxide?
In a compound the ratio of the atoms or element by mass remains always same irrespective of :
If the ratio of the atoms by mass is altered then :
Law of constant proportion states that :
Hydrogen combines with oxygen to form water. Water exists in:
Hydrogen combines with oxygen to form $H _2O$ in which 16 g of oxygen combine with 2 g of hydrogen. Hydrogen also combines with carbon to form $CH _4$ in which 2 g of hydrogen combine with 6 g of carbon.If carbon and oxygen combine together then they will do show in the ratio of
Two gases found dissolved in natural water are
A sample of pure carbon dioxide, irrespective of its source contains 27.27 % carbon and 72.73% oxygen. The given data supports:
In Haber's process, the volume of ammonia relative to the total volume of reactants at STP is:
$2.16$ grams of Cu, on reaction with $HNO _{3}$, followed by ignition of the nitrate, gave $2.7$ g of copper oxide. In another experiment $1.15$ g of copper oxide, upon reaction with hydrogen, gave $0.92$ g of copper. This data illustrate the law of:
An experiment showed that a lead chloride solution is formed when 6.21 g of lead combines with 4.26 g of chlorine. What is the empirical formula of this chloride?
Common salt obtained from Clifton beach contained $60.75\%$ chlorine while $6.40$ g of a sample of common salt from Khewra mine contained $3.888$ g of chlorine. State the law illustrated by these chemical combinations.
A sample of calcium carbonate $\displaystyle \left ( CaCO _{3} \right )$ has the percentage composition as given: $Ca = 40\%,\ C = 12\%,\ O = 48\%$.
1.2375 g of cupric oxide on being heated in a current of hydrogen gave 0.9322 g of the metal In another experiment 0.9369 g of pure copper was dissolved in nitric acid Excess of acid evaporated and the residue has ignited The weight of the cupric oxide left was 1.2469 g. Which law of chemical combination is shown by the above results?
The percentage of copper and oxygen in a sample of CuO obtained from different methods were found to be same. This proves the law of :
$1.375$ g of cupric oxide was reduced by heating in a current of hydrogen and the weight of copper obtained was $1.098$ g. In another experiment, $1.156$ g of copper was dissolved in nitric acid and the resulting solution was evaporated to dryness. The residue of copper nitrate when strongly heated was converted into $1.4476$ g of cupric oxide. State the law illustrated by these chemical combinations.
A pair of compounds which is an illustration of law of multiple proportions is:
Any sample of pure water, irrespective of its source, contains 88.89% oxygen and 11.11 % hydrogen by mass. The data supports the:
Hydrogen combines with nitrogen in a 3:14 weight ratio to form ammonia. If every molecule of ammonia contains three atoms of hydrogen and one atom of nitrogen, an atom of nitrogen must weigh :
Hydrogen combines with oxygen in a 1:8 weight ratio to form water. If every molecule of water contains two atoms of hydrogen and one atom of oxygen, an atom of oxygen must weigh :
When elements react, their atoms combine in :
When $3\ g$ of carbon is burnt in $8\ g$ of oxygen, $11 g$ of carbon dioxide is produced. What mass of carbon dioxide will be formed when $3\ g$ of carbon is burnt in $50\ g$ oxygen?
When $1.375\ g$ of cupric oxide is reduced on heating in a current of hydrogen, the weight of copper remaining $1.098\ g$. In another experiment, $1.179\ g$ of copper is dissolved in nitric acid and resulting copper nitrate converted into cupric oxide by ignition. The weight of cupric oxide formed is $1.476 \ g$. This is in agreement with :
Who stated the law of constant proportion?
A 78.0 g sample of an unknown compound contains 12.4 g of hydrogen. What is the percent by mass of hydrogen in the compound?
The percentage of copper and oxygen in samples of CuO obtained by different methods were found to be the same. This illustrates the law of:
Which of the following statement is incorrect for the composition of water?
Nitrogen reaction with oxygen to form nitrogen (III) oxide.
A sample of $CaCO _3$ has Ca - 40%, C = 12% and 0 = 48%. If the law of constant proportions is true, then the mass of Ca in 5 g of $CaCO _3$ from another source will be:
Potassium combines with two isotopes of chlorine $(^{35} Cl\,\, and\,\, ^{37}Cl)$ respectively to form two samples of $KCl$ Their formation follows the law of:
In the reaction, $N _2 + 3H _2 \rightarrow 2NH _3$, the ratio of volumes of nitrogen, hydrogen and ammonia is 1 : 3: 2. These figures illustrate the law of:
The law of constant proportions was enunciated by:
Zinc sulphate contains 22.65% Zn and 43.9% $H _2O$. If the law of constant proportions is true, then the mass of zinc required to give 40 g crystals will be:
3 volumes of hydrogen are required to combine with one volume of nitrogen to form 2 volumes of ammonia. When 1 mole of hydrogen is allowed to react with the mole of nitrogen, the two gases?
If a mixture containing 3 moles of hydrogen and 1 mole of nitrogen is converted completely into ammonia, the ratio of initial and final volumes under the same temperature and pressure would be:
If water samples are taken from the sea, rivers, clouds, lakes or snow, they will be found to contain hydrogen and oxygen in the ration of $1 : 8$. This clearly demonstrates the law of ?
If you put a waterproof, nine-volt battery in a mug of water containing two teaspoonfuls of salt, the water will be broken into gases and bubbles will start forming. What are these gases?
A sample of pure water, irrespective of source, contains 88.89% oxygen and 11.11% hydrogen
by mass. The data supports the:
When one mole each of CO and $O _2$ are made to react at STP, the total number of moles at an end of the reaction is:
64g of an organic compound has 24 g carbon and rest hydrogen and oxygen. The empirical formula of the compound is
Zinc sulphate contains $22.65$% $Zn$ and $43.9$% ${H} _{2}O$. If the law of constant proportions is true, then the mass of zinc required to give $40g$ crystal will be:
Which of the following statements is/are correct?
$14$ g of element X combines with $16$ g of oxygen. On the basis of this information, which of the following is a correct statement?
The % loss in mass after heating a pure sample of potassium chlorate (Mol. mass = 122.5) will be:
The volume of oxygen at NTP evolved when 1.70 g of sodium nitrate is heated to a constant mass is:
The mass of residue left after strongly heating 1.38 g of silver carbonate will be:
At NTP, 10 litre of hydrogen sulphide gas reacted with 10 litre of sulphur dioxide gas. The volume of gas, after the reaction is complete, would be:
Which of the following is a limitation of the law of constant composition is not applicable?
Statement: Every nine parts of water by weight contain eight parts by weight of oxygen.