Observe the following reactions (unbalanced): | vedclass

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(D) The balanced chemical equations are:$P_2O_3 + 3H_2O \rightarrow 2H_3PO_3$ $(X = H_3PO_3)$$P_4O_{10} + 6H_2O \rightarrow 4H_3PO_4$ $(Y = H_3PO_4)$I

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$1, 1$

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(D) The balanced chemical equations are:$P_2O_3 + 3H_2O \rightarrow 2H_3PO_3$ $(X = H_3PO_3)$$P_4O_{10} + 6H_2O \rightarrow 4H_3PO_4$ $(Y = H_3PO_4)$In $H_3PO_3$ (phosphorous acid), the structure contains $1$ $P=O$ bond, $2$ $P-OH$ bonds, and $1$ $P-H$ bond.In $H_3PO_4$ (phosphoric acid), the structure contains $1$ $P=O$ bond and $3$ $P-OH$ bonds.Thus, the number of $P=O$ bonds in $X$ and $Y$ are $1$ and $1$ respectively.

Observe the following reactions (unbalanced):
$P_2O_3 + H_2O \rightarrow X$
$P_4O_{10} + H_2O \rightarrow Y$
The number of $P=O$ bonds present in $X$ and $Y$ are respectively:

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Observe the following reactions (unbalanced):$P_2O_3 + H_2O \rightarrow X$$P_4O_{10} + H_2O \rightarrow Y$The number of $P=O$ bonds present in $X$ and $Y$ are respectively: