Home
Class 11
CHEMISTRY
Element X and Y form two different compo...

Element `X` and `Y` form two different compounds. In the first compound, `0.324 g X` is combined with `0.471 g Y`. In the second compound, `0.117 g X` is combined with `0.509 g Y`. Show that these data illusttate the law of multiple proportions.

Text Solution

AI Generated Solution

To demonstrate that the data provided illustrates the law of multiple proportions, we will follow these steps: ### Step 1: Understand the Law of Multiple Proportions The law of multiple proportions states that when two elements combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element can be expressed as a ratio of small whole numbers. ### Step 2: Collect the Given Data We have two compounds formed by elements X and Y: - **Compound 1**: 0.324 g of X combines with 0.471 g of Y ...
Promotional Banner

Topper's Solved these Questions

  • SOME BASIC CONCEPTS AND MOLE CONCEPT

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 1.1 Objective Questions|6 Videos

  • SOME BASIC CONCEPTS AND MOLE CONCEPT

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 1.1 Objective Questions (Single Correct)|3 Videos

  • S-BLOCK GROUP 2 - ALKALINE EARTH METALS

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 5.1 Objective|2 Videos

  • STATES OF MATTER

    CENGAGE CHEMISTRY ENGLISH|Exercise Exercises (Ture False)|25 Videos

Similar Questions

Explore conceptually related problems

Hydrogen combines with oxygen and forms two compounds. In the first compound, hydrogen content is 5.93% while in the other compound it is 11.2%. Verify whether the data agrees with law of multiple proportions.

metal combines with oxygen to form two oxides, having the following composition: (i) 0.398 g of the first metal oxide contains 0.318g of metal. (ii) 0.716 g of the second oxide contains 0.636g of the metal. Show that the above data agrees with the law of multiple proportions.

Elen A and B combine to form three different compounds: 0.3 g of A + 0.4 g of B rarr 0.7 g of compound X 18.0 g of A + 48.0 g of B rarr 66.0 g of compound Y 40.0 g of A + 159.99 g of B rarr 199.99 g of compound Z Show that the law of multiple proportions is illustrated by the data given above.

This law was proposed by Dalton in 1803 . According to this law , if two elements combune to form more than one compounds ,the masses of one element that combine with a fixed mass of the other element, are in the ratio of small whole number. For exemple, hydrogen combines with oxygen to form two compounds ,namely, water and hydrogen peroxide. Here, the masses of oxygen (i.e, 16g and 32g) which combine with a fixed mass of hydrogen (2g) bear a simple raio, i.e, 16 :32 or 1 :2 . An element forms two oxides .In one oxide ,one gram of the oxide containd 0.5g of the element. In another oxide, 4g of the oxide contains 0.8g of the element . Show that these data confirm the law of multiple proportion.

Two elements P and Q combine to form two different compounds in stoichimetric ratios of 1:2 and 1:3.If 0.25 mole of 1^(st) compound weighs 16 g and 0.05 mole of 2^(nd) compound weighs 4 g, then the atomic weighs of P and Q respectively are

3.2 g sulphur combines with 3.2 g of oxygen, to from a compound in one set of conditions. In another set of conditions 0.8 g of sulphur combines with 1.2 g of oxygen to form another compound. State the law illustrated by these chemical combinations.

Two elements X and Y combine to form a compound XY. Under what conditions the bond formed between them will be ionic ?

This law was proposed by Dalton in 1803 . According to this law , if two elements combune to form more than one compounds ,the masses of one element that combine with a fixed mass of the other element, are in the ratio of small whole number. For exemple, hydrogen combines with oxygen to form two compounds ,namely, water and hydrogen peroxide. Here, the masses of oxygen (i.e, 16g and 32g) which combine with a fixed mass of hydrogen (2g) bear a simple raio, i.e, 16 :32 or 1 :2 0.11 g of an oxide of nitrogen gives 56 Ml N_(2) at 273K and 1 atm. 0.15 g of another oxide of nitrogen gives 56mL N_(2) at 1 atm , 273K. Show that these data confirm the law of multiple proportion.

A metal forms two oxides. The higher oxide contains 80% metal. 0.72 g of the lower oxide gave 0.8 g of higher oxide when oxidised. Calculate the weight of oxygen the combines with the fixed weight of metal in the two oxides, and show that the data supports the law of multiple proportines

An element X burns in oxygen to form an electrovalent compound XO. What is the formula of compounds formed if this element is allowed to combine with chlorine