Zn + 2HCl → ZnCl_2 + H_2 1 mole 2 moleso, if Zn = 0.2 mole ⇒ HCl = 0.1 mole #160;no. of moles = wtmol.wt 1 = wt of HClmol wt of HCl w ...

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Standard X

Chemistry

Application of Electrolysis

What mass of ...

Question

What mass of 60% HCl (by mass) is required to completely react with 0.2 mol of zinc and what volume of $H_{2}$ will be produced at S.T.P.? The reaction is
$Z n + 2 H C l \to Z n {C l}_{2} + H_{2}$

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Solution

$Z n + 2 H C l \to Z n C l_{2} + H_{2}$
1 mole 2 mole
so, if Zn = 0.2 mole
$\Rightarrow$ HCl = 0.1 mole
no. of moles = $\frac{w t}{m o l . w t}$
$1 = \frac{w t o f H C l}{m o l w t o f H C l}$
wt of HCl = $0.1 \times 36.5$
=3.65 g
60 % of HCl = 2.19 g
1 mole of gas has 22.4L vol
here, 1 mole of Zn will
give 1 mole of $H_{2}$
here, 0.2 moles of $H_{2}$
means, $2 * 22.4 L$
= $4.48 L$ of $H_{2}$

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What mass of 60% HCl (by mass) is required to completely react with 0.2 mol of zinc and what volume of H2 will be produced at S.T.P.? The reaction is Zn+2HCl→ZnCl2+H2

Zn+2HCl→ZnCl2+H21 mole 2 moleso, if Zn = 0.2 mole⇒ HCl = 0.1 mole no. of moles = wtmol.wt1=wtofHClmolwtofHClwt of HCl = 0.1×36.5=3.65 g60 % of HCl = 2.19 g1 mole of gas has 22.4L volhere, 1 mole of Zn willgive 1 mole of H2here, 0.2 moles of H2means, 2∗22.4L= 4.48L of H2

What mass of 60% HCl (by mass) is required to completely react with 0.2 mol of zinc and what volume of $H_{2}$ will be produced at S.T.P.? The reaction is
$Z n + 2 H C l \to Z n {C l}_{2} + H_{2}$