Match the following:

Column I	Column II
(i) 88 g of CO2	(a) 0.25 mol
(ii) 6.022×1023  molecules of H2O	(b) 2 mol
(iii) 5.6 litres of O2 at STP	(c) 1 mol
(iv) 96 g of O2	(d) 6.022×1023 molecules
(v) 1 mol of any gas	(e) 3 mol

<p>This is a Matching Type Questions as classified in NCERT Exemplar</p><p> (i)- (b); (ii) - (c); (iii) - (a); (iv) - (e); (v) - (d)</p><p><strong> (i)</strong> 88 g of CO₂</p><p>The number of moles is given by the following formula, </p><p>Moles =<span contenteditable="false"> <math> <mfrac> <mrow> <mrow> <mi mathvariant="normal">M</mi> <mi mathvariant="normal">a</mi> <mi mathvariant="normal">s</mi> <mi mathvariant="normal">s</mi> </mrow> </mrow> <mrow> <mrow> <mi mathvariant="normal">M</mi> <mi mathvariant="normal">o</mi> <mi mathvariant="normal">l</mi> <mi mathvariant="normal">a</mi> <mi mathvariant="normal">r</mi> <mi mathvariant="normal"> </mi> <mi mathvariant="normal">m</mi> <mi mathvariant="normal">a</mi> <mi mathvariant="normal">s</mi> <mi mathvariant="normal">s</mi> <mi mathvariant="normal"> </mi> <mi mathvariant="normal"> </mi> <mi mathvariant="normal"> </mi> <mi mathvariant="normal"> </mi> <mi mathvariant="normal"> </mi> </mrow> </mrow> </mfrac> </math> </span> &nbsp;- (1)</p><p>So, the number of moles of CO₂ is calculated by using equation (1) as follows</p><p>Moles of CO₂= <span contenteditable="false"> <math> <mfrac> <mrow> <mrow> <mn>88</mn> <mi mathvariant="normal"> </mi> <mi mathvariant="normal">g</mi> </mrow> </mrow> <mrow> <mrow> <mn>44</mn> <mi mathvariant="normal"> </mi> <mi mathvariant="normal">g</mi> <mi mathvariant="normal"> </mi> <mo>/</mo> <mi mathvariant="normal"> </mi> <mi mathvariant="normal">m</mi> <mi mathvariant="normal">o</mi> <mi mathvariant="normal">l</mi> <mi mathvariant="normal"> </mi> <mi mathvariant="normal"> </mi> <mi mathvariant="normal"> </mi> </mrow> </mrow> </mfrac> </math> </span>= 2 mol</p><p>Thus, option (i) from column I is matched with (b) from column II</p><p><strong> (ii)</strong>&nbsp; 1 mol of H₂O gives 6.022*10²³&nbsp;molecules. So, 6.022*10²³&nbsp;molecules contain 1 mol of H₂O . Thus, option (ii) from column I is matched with (b) from column II</p><p><strong> (iii)</strong> 5.6 liters of O₂ at STP</p><p>1 mol of gas occupies 22.4 liters of O2 . For 5.6 liters of O₂, the number of moles of oxygen gas is calculated as</p><p>Moles of O₂ = <span contenteditable="false"> <math> <mfrac> <mrow> <mrow> <mn>88</mn> <mi mathvariant="normal"> </mi> <mi mathvariant="normal">g</mi> </mrow> </mrow> <mrow> <mrow> <mn>22.4</mn> <mi mathvariant="normal"> </mi> <mi mathvariant="normal">L</mi> <mi mathvariant="normal"> </mi> <mi mathvariant="normal"> </mi> <mi mathvariant="normal"> </mi> </mrow> </mrow> </mfrac> </math> </span>&nbsp;* 5.6 L = 0.25 mol</p><p> (iv) 96 g of O₂</p><p>The number of moles of O₂ is calculated by using equation (1) as follows, </p><p>Moles of O₂ = <span contenteditable="false"> <math> <mfrac> <mrow> <mrow> <mn>96</mn> <mi mathvariant="normal"> </mi> <mi mathvariant="normal">g</mi> </mrow> </mrow> <mrow> <mrow> <mn>32</mn> <mi mathvariant="normal"> </mi> <mi mathvariant="normal">g</mi> <mi mathvariant="normal"> </mi> <mo>/</mo> <mi mathvariant="normal"> </mi> <mi mathvariant="normal">m</mi> <mi mathvariant="normal">o</mi> <mi mathvariant="normal">l</mi> <mi mathvariant="normal"> </mi> <mi mathvariant="normal"> </mi> </mrow> </mrow> </mfrac> </math> </span>&nbsp;= 3 mol</p><p>Thus, option (iv) from column I is matched with (e) from column II.</p><p> (v) 1 mol of any gas 1 mole of any gas contains 6.022*10²³&nbsp;molecules.</p><p>Thus, option (v) from column I is matched with (d) from column II.</p>

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