Calculate the mass of copper(II) oxide required when reacts with excess sulfuric acid to form 1 mol of $C u S O_{4}$ . The equation for the reaction is:

$C u O + H_{2} S O_{4} \to C u S O_{4} + H_{2} O$

[Given $: C u = 63.5; O = 16; S = 32$ ]

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Solution

According to equation,
1 mole of CuO reacts with 1 mole of $H_{2} S O_{4}$

If excess of sulfuric acid is there, then complete 1 mole of CuO will react
so, mass of CuO react = 63.5 + 16 = $79.5 g$

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Similar questions

2.5 g

C u O + H_{2} {S O}_{4} \to {C u S O}_{4} + H_{2} O

What is the balanced form of the equation written below?

$C u + H_{2} S O_{4} \to C u S O_{4} + S O_{2} + H_{2} O$

C u {S O}_{4}

Z n + C u {S O}_{4} ⟶ Z n {S O}_{4} + C u

100 m l

0.05 M

C u {S O}_{4}

C u S O_{4} .5 H_{2} O \to C u S O_{4} + 5 H_{2} O

C u S O_{4} + 2 K C N \to C u (C N)_{2} + K_{2} S O_{4}

2 C u (C N)_{2} \to 2 C u C N + (C N)_{2}

2 C u C N + 6 K C N \to 2 K_{3} [C u (C N)_{4}]

(Molar mass of K = 39 g / m o l, C u = 63.5 g / m o l)

{C u S O}_{4}

Z n + {C u S O}_{4} \to {Z n S O}_{4} + C u

{C u S O}_{4}

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