In an experiment $1.288 g$ of copper oxide was obtained from $1.03 g$ of copper and $0.258 g$ of oxygen. Calculate the ratio of copper and oxygen in the sample?

Open in App

Solution

$2 C u + O_{2} \to 2 C u O$

$1.03 g$ $0.258 g$ $1.288 g$

Therefore, since $M a s s o f r e a c t a n t s = M a s s o f p r o d u c t s$ . It is following the law of conservation of mass.

$\frac{R a t i o o f C o p p e r}{R a t i o o f O x y g e n} = \frac{1.03}{0.258} = \frac{3.99}{1} = 4 : 1$

Suggest Corrections

Similar questions

Q. In two different experiments, the copper oxide was obtained from copper. The ratio of the mass of copper and the mass of oxygen found in the two experiments are the same. They are in the ratio of

4 : 1

. What of you infer about the experiments?

Q. In an experiment, 4.90 g of copper oxide was obtained from 3.92 g of copper. In another experiment, 4.55 g of copper oxide gave, on reduction, 3.64 g of copper. Show with the help of calculations that these figures verify the law of constant proportions.

Q. In an experiment, 1.288 g of copper oxide was obtained from 1.03 g of copper. In another experiment, 3.672 g of copper oxide gave, on reduction, 2.938 g of copper. Show that these figures verify the law of constant proportions.

In a experiment, 4.90g of copper oxide was obtained from 3.92g of copper. In another experiment, 4.55g copper oxide gave on reduction 3.64g of copper. Show that these figures verify the law of constant proportion.

Join BYJU'S Learning Program

In an experiment 1.288 g of copper oxide was obtained from 1.03 g of copper and 0.258 g of oxygen. Calculate the ratio of copper and oxygen in the sample?

2Cu+O2→2CuO1.03g 0.258g 1.288gTherefore, since Mass of reactants=Mass of products. It is following the law of conservation of mass.Ratio of CopperRatio of Oxygen=1.030.258=3.991=4:1

In an experiment $1.288 g$ of copper oxide was obtained from $1.03 g$ of copper and $0.258 g$ of oxygen. Calculate the ratio of copper and oxygen in the sample?

$2 C u + O_{2} \to 2 C u O$

$1.03 g$ $0.258 g$ $1.288 g$

Therefore, since $M a s s o f r e a c t a n t s = M a s s o f p r o d u c t s$ . It is following the law of conservation of mass.

$\frac{R a t i o o f C o p p e r}{R a t i o o f O x y g e n} = \frac{1.03}{0.258} = \frac{3.99}{1} = 4 : 1$