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In air, element X is oxidised to compoun...

In air, element X is oxidised to compound `XO_(2)`, . If 1.0 gram of X reacts with 0.696 g of oxygen, what is the atomic weight of X?

Text Solution

AI Generated Solution

To find the atomic weight of element X that is oxidized to form the compound \(XO_2\), we can follow these steps: ### Step 1: Write the balanced chemical equation The reaction can be represented as: \[ X + O_2 \rightarrow XO_2 \] ...
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Knowledge Check

  • Element 'A' reacts with oxygen to form a compound A_(2)O_(3) . If 0.359 gram of 'A' react to give 0.559 gram of the compound, atomic weight of 'A' will be

    A
    51
    B
    43.08
    C
    49.7
    D
    47.9

  • Element X reacts with oxygen to form a compound, whose simplest formula is X_2O_3. If 0.359 g of X react to give 0.559 g of the compound, atomic weight of X is found to be

    A
    47.9 amu
    B
    49.7 amu
    C
    43.08 amu
    D
    51.0 amu

  • An element X forms an oxide XO_(3) . What is the valency of X?

    A
    1
    B
    2
    C
    3
    D
    6

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    A 2.18 g sample contains a mixture of XO and X_(2)O_(3) . It reacts with 0.015 moles of K_(2)Cr_(2)O_(7) to oxidize the sample completely to form XO_(4)^(-) " and " Cr^(3+) . If 0.0187 mole of XO_(4)^(-) is formed , what is the atomic mass of X ?

    You are given a 2.198 - g sample containing a mixture of XO and X_(2)O_(3) .It requires 0.015 mol of K_(2)Cr_(2)O_(7) to oxidise the sample completely to form XO_(4)^(-) and Cr^(3+) .If 0.0817 mole XO_(4)^(-) is formed ,what is the atomic mass of X?

    An element A (atomic weight = 12) and B (atomic weight = 35.5) combines to form a compound X. If 4 mol of B combines with 1 mol of A to give 1 mol of X. The weight of 1 mol of X would be :

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    Element X reacts with oxygen to produce a pure sample of X_2 O_3 . In a experiment, it is found that 1.00 g of X produces 1.16g of X_2 O_3 . What will be the atomic mass of X.

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