Home
Class 11
CHEMISTRY
1.375 g of cupric oxide was reduced by h...

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

Text Solution

Verified by Experts

First case :
Copper oxide taken `= 1.375 g`
Copper left `= 1.098 g`
`:.` Oxygen present `= 1.357 g - 1.098 = 0.277 g`
Hence, % of `O_(2)` in `CuO = (0.277 xx 100)/(1.357) = 20.14`
second case :
Copper taken `= 1.179 g`
Copper oxide formed `= 1.476 g`
`:.` Oxygen present `= 1.476 g - 1.179 = 0.297 g`
Hence, % of `O_(2)` in `CuO = (0.297 xx 100)/(1.476) = 20.12`
Hence, percentage of oxygen is same in both of the above cases, so the is proved.
Promotional Banner

Similar Questions

Explore conceptually related problems

4 g of copper was dissolved in concentrated nitric acid. The copper nitrate on strong heating gave 5 g of its oxide. The equivalent weight of copper is

Weight of copper oxide obtained by heating 2.16 g of metallic copper with HNO_(3) and subsequent ingnition was 2.70 g In another experient, 1.15 g of copper oxide on reduction yielded 0.92 g of copper. Show that the results illustrance the law of definite proportions.

1.0 g of an oxide of metal M contained 0.5 g of M and 4.0 g of another oxide of M contained 1.6 g of M. These data illustrate the

112 mL of hydrogen combines with 56 mL of oxygen of form water. When 224 mL of hydrogen is passes over hand cupric oxide, the cupric oxide loses. 0.160 g of weight. All volumes are measured at STP . Show that the result agrees with the law of constant composition (22.4 L hydrogen and oxygen at STP weigh, respectively, 2g and 32 g )

0.22 g of a hydrogen (i.e., a compound conatining carbon and hydrogen only) on complete combustion with oxygen gave 0.9 g water and 0.44 g carbon dioxide. Show that these results are in accordance with the law of conservation of mass (atomic mass of C = 12, H = 1, O = 16) .

An electric current is passed through three cells in series containing respectively solutions of copper sulphate, silver nitrate and potassium iodide. What weights of silver and iodine will be liberated while 1.25 g of copper is being deposited ?

What weight of sodium chloride would be decomposed by 4.9 g of sulphric acid, if 6 g of sodium bisulphate (NaHSO_(4)) and 1.825 g of hydrogen chloride were produced in the reaction and the law of conservation of mass is true?

1 g of oxygen combines with 0.1260 g of hydrogen to form H_(2)O . 1 g of nitrogen combines with 0.2160 g of hydrogen to form NH_(3) . Predict the weight of oxygen required to combine with 1 g of nitrogen to form an oxide.

If the law of constant compositon is true, what weights of calcium carbon, and oxygen are present in 1.5 g of calcium carbonate, if a sample of calcium carbonate from another source contains the following percentage composition: Ca = 40.0%, C = 12.0% , and O = 48.0% ?