Question

2.16 g of a metal oxide on strong heating produced 112 ml of oxygen at STP and the residue was pure metal calculate the equivalent weight of the metal​

Answer 1

Answer:

The equivalent weight of metal will be 200.

Explanation:

The mass of metal oxide is 2.16g.

The volume of oxygen formed from the metal oxide is 112mL.

we know that:

$1000mL=1L$

$112mL=0.112L$

at STP

The 22.4L of volume is occupied by one mole of a gas.

The moles of oxygen formed will be:

$\frac{0.112}{22.4}=0.005mol$

The number of gram equivalents of oxygen will be:

$=0.005X2=0.01$

The mass of oxygen in 2.16g of metal oxide =$molesXmolarmass=0.005X32=0.16g$

$The mass of metal in the metal oxide=2.16-0.16=2.00g$

The equivalents of the two will be the same

So the equivalent weight of metal will be = $\frac{mass}{no.ofgramequivalents}=\frac{2}{0.01}=200$

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