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A current is passed through two cells co...

A current is passed through two cells connected in series. The first cell contains `X(NO_(3))_(3(aq))` and the second cell contains `Y(NO_(3))_(2(aq))` . The relative atomic masses of X and Y are in the ratio `1:2`. What is the ratio of liberated mass of X to that of Y ?

Answer

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A current is passed through two cells connected in series. The first cell contains X(NO_(3))_(3)(aq) and the second cell contains Y(NO_(3))_(2)(aq) . The relative atomic masses of X and Y are in the ratio 1:2. what is the ratio of the liberated mass of X to that of Y?

Certain quantity of current is passed through 2 voltameters connected in series and containing XSO_4 (aq) and Y_2SO_4 (aq) respectively. If the atomic masses of X and Y are in the ratio of 2 : 1 the ratio of the masses of Y liberated to that of X is

Knowledge Check

  • A current is passed through two cells connected in series. The first cell contains X(NO_(3))_(3)(aq) and the second cell contains Y(NO_(3))_(2)(aq) . The relative atomic masses of X and Y are in the ratio 1:2, what is the ratio of the liberated mass of X to that of Y?

    A
    `3:2`
    B
    `1:2`
    C
    `1:3`
    D
    `3:1`

  • Current is passed through two cells connected in series, the first cell contains X(NO_3)_(3(aq)) and the second cell contains Y(NO_(3))_(2(aq)) . The relative atomic masses of X and Y are in the ratio 1 : 2. What is the ratio of the liberated mass of X to that of Y?

    A
    `3:2`
    B
    `1:2`
    C
    `1:3`
    D
    `3:1`

  • A current is passed through two cells connected in series. The first cell contain x(NO_(3))_(2) (aq) and the second cell contains y(NO_(3))_(2)(aq) . The relative atomic masses of x and y are in the ratio of x to that of y?

    A
    `3:2`
    B
    ` 1:2`
    C
    `1:3`
    D
    ` 3:1`

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    In an electrolysis experiment, a current was passed for 5 hourss through two cells connected in series. The first cell contains a solution of gold salt and the second cell contains copper sulphate solution. 9.85 g of gold was deposited in the first cell. If the oxidation number of gold is +3, find the amount of copper deposited on the cathode in the second cell. Also calculate the magnitude of the current in ampere.

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