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.

Element X reacts with oxygen to produce a pure sample of X_(2)O_(3) . In an experiment it is found that 1.00g of X produces 1.16g" of "X_(2)O_(3) . Calculate the atomic weight of X. (Atomic weight of oxygen, 16.0 gmol^(-1) ).

5.0 g of a certain element X forms 10.0 g of its oxide having the formula X_4O_6 . What is the atomic mass of X

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

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?

An alloy of metals X and Y weighs 12 g and contains atoms X and Y in the ratio of 2:5. The percentage by mass of X in the sample is 20. If atomic mass of X is 40, what is the atomic mass of metal Y?