What mass of zinc metal is required to evolve a $30 \cdot m L$ $30mL$ volume of dihydrogen gas from a $30 \cdot m L$ $30mL$ volume of hydrochloric acid at $1.00 \cdot m o l \cdot L^{- 1}$ $1.00molL^-1$ concentration?

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What mass of zinc metal is required to evolve a $30 \cdot m L$ $30mL$ volume of dihydrogen gas from a $30 \cdot m L$ $30mL$ volume of hydrochloric acid at $1.00 \cdot m o l \cdot L^{- 1}$ $1.00molL^-1$ concentration?

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Answer 1 · 2016-03-03T06:26:04

From the equation you can see that one mole of Zn will react with two moles of HCl.

Explanation:

Calculate the number of moles of HCl in 30mL of 1.00M solution, and divide by 2 for moles of Zn. Then multiply that by the molecular weight of Zn.

1M = 1mole/L 0.030L * 1mole/L = 0.030 moles HCl. 0.015 moles of Zn will react.

Answer 2 · 2016-03-03T06:33:44

Nearly $1$ $1$ $gram$ $"gram"$ zinc metal is required.

Explanation:

$Z n (s) + 2 H C l (a q) \to Z n C l_{2} (a q) + H_{2} (g) ↑ ⏐$ $Zn(s) + 2HCl(aq) rarr ZnCl_2(aq) + H_2(g)uarr$ .

Each equiv of zinc metal requires 2 equiv of hydrochloric acid for complete oxidation. This gives this molar quantity: we simply take half of the molar quantity of hydrochloric acid used.

$n_{H C l}$ $n_(HCl)$ $=$ $=$ $30 \times 10^{- 3} L \times 1.00 \cdot m o l \cdot L^{- 1}$ $30xx10^-3Lxx1.00*mol*L^-1$ $=$ $=$ $? ?$ $??$

$n_{H C l}$ $n_(HCl)$ $=$ $=$ $\frac{n_{Z n}}{2}$ $n_(Zn)/2$ .

So the mass of zinc is simply:

$30 \times 10^{- 3} L \times 1.00 \cdot m o l \cdot L^{- 1} \times \frac{1 equiv of zinc}{2 equiv of acid} \times 65.38 \cdot g \cdot m o l^{- 1}$ $30xx10^-3Lxx1.00*mol*L^-1xx("1 equiv of zinc")/("2 equiv of acid")xx65.38*g*mol^-1$ $=$ $=$ $? ? g$ $??g$

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What mass of zinc metal is required to evolve a $30 \cdot m L$ $30mL$ volume of dihydrogen gas from a $30 \cdot m L$ $30mL$ volume of hydrochloric acid at $1.00 \cdot m o l \cdot L^{- 1}$ $1.00molL^-1$ concentration?

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What mass of zinc metal is required to evolve a 30⋅mL30*mL volume of dihydrogen gas from a 30⋅mL30*mL volume of hydrochloric acid at 1.00⋅mol⋅L−11.00*mol*L^-1 concentration?

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What mass of zinc metal is required to evolve a $30 \cdot m L$ $30mL$ volume of dihydrogen gas from a $30 \cdot m L$ $30mL$ volume of hydrochloric acid at $1.00 \cdot m o l \cdot L^{- 1}$ $1.00molL^-1$ concentration?