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X + 2Y → XY2


If X and Y are completely consumed in the reaction and we start with 10.0 mol of Y, then how many total moles of X and Y will be in the reaction?
A) 5.0 mol
B) 10.0 mol
C) 15.0 mol
D) 20.0 mol

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Edufirst

Answer:

                         [tex]\large\boxed{\large\boxed{OptioncC)15.0mol}}[/tex]

Explanation:

The reaction between hypothetical elements X and Y to produce hypothetical compound XY₂ is represented with the chemical equation:

  • X + 2Y → XY₂

That equation means that one atom (or one mole of atoms) of element X reacts with 2 atoms (or two moles of atoms) of element Y to produce one molecule (one mole of molecules) of compound XY₂.

Elements X and Y are the reactants, and compound XY₂ is the product.

Hence, the mole ratio is:

  • 1 mol X : 2 mol Y : 1 mol XY₂

Since, 10.0 mol of Y completely react you can set the corresponding proportions with X and XY₂ to find how many moles of them will be in the reaction:

1. Moles of X:

  • Theoretical ratio: 1 mol of X / 2 mol of Y

  • Ratio with 10.0 mol of Y: U / 10.0 mol of Y

  • Proportion: equal the two ratios: 1 mol X / 2 mol Y = U / 10.0 mol Y

  • Solve for U: U = 10.0 mol Y × 1 mol X / 2 mol Y = 5.0 mol X

  • Result: 5.0 moles of X are in the reaction.

2. Total moles of X and Y in the reaction:

  • The total number of moles is the sum of the moles of the two reactants: 10.0 moles of Y + 5.0 moles of X = 15.0 moles. Hence 15.0 mol of X and Y are in the reaction: option C).

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