Suppose the elements X and Y combine to form | vedclass

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(A) For $XY_2$: $0.1 \ mol$ of $XY_2 = 10 \ g$ $1 \ mol$ of $XY_2 = 100 \ g$ So,$X + 2Y = 100$ (Equation $1$) For $X_3Y_2$: $0.05 \ mol$ of $X_3Y_2 =

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$40, 30$

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(A) For $XY_2$: $0.1 \ mol$ of $XY_2 = 10 \ g$ $1 \ mol$ of $XY_2 = 100 \ g$ So,$X + 2Y = 100$ (Equation $1$) For $X_3Y_2$: $0.05 \ mol$ of $X_3Y_2 = 9 \ g$ $1 \ mol$ of $X_3Y_2 = 180 \ g$ So,$3X + 2Y = 180$ (Equation $2$) Subtracting Equation $1$ from Equation $2$: $(3X + 2Y) - (X + 2Y) = 180 - 100$ $2X = 80 \implies X = 40$ Substituting $X = 40$ in Equation $1$: $40 + 2Y = 100$ $2Y = 60 \implies Y = 30$ Therefore,the atomic weights of $X$ and $Y$ are $40$ and $30$ respectively.

Suppose the elements $X$ and $Y$ combine to form two compounds $XY_2$ and $X_3Y_2.$ When $0.1 \ mol$ of $XY_2$ weighs $10 \ g$ and $0.05 \ mol$ of $X_3Y_2$ weighs $9 \ g,$ the atomic weights of $X$ and $Y$ are

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