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2 years ago

What mass of hydrogen is produced when 192 g of magnesium is reacted with hydrochloric acid?

Chemistry

2 answers:

Leona [35]2 years ago

5 0

$\huge\underline{\underline{\boxed{\mathbb {SOLUTION:}}}}$

$\longrightarrow \sf{Mg+2HCI \Longrightarrow MgCl_2+H_2}$

$\longrightarrow \sf{molMg=129gMg \times \dfrac{1molMg}{24.305gMg=} }$

$\small \sf{\longrightarrow molH_2=7.90molMg \times \dfrac{1molH_2}{1molMg}= 7.90molH_2 }$

$\small \sf{\longrightarrow massH_2=7.90H_2 \times \dfrac{2.016g}{1molH_2}= 7.90molH_2= 15.9 \: gH_2}$

$\huge\underline{\underline{\boxed{\mathbb {ANSWER:}}}}$

$\small\bm{ The \: mass \: of \:H_2 \: produce \: will \: be \: 15.9 }$ $\bm{grams.}$

mariarad [96]2 years ago

3 0

Answer:

Mg+2HCL-Magnesium Chloride +Hygrogen

$>$

Explanation:

N.O of moles=Mass\Molar Mass

192÷24=8

1:1

8×2=16

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$P\cdot V = n\cdot R_{u}\cdot T$ (1)

$P\cdot V = \frac{r\cdot R_{u}\cdot T}{N_{A}}$ (1b)

Where:

$P$ - Pressure, measured in pascals.

$V$ - Volume, measured in liters.

$r$ - Amount of molecules, no unit.

$N_{A}$ - Avogadro's number, no unit.

$R_{u}$ - Ideal gas constant, measured in pascal-liters per mole-Kelvin.

$T$ - Temperature, measured in Kelvin.

If we know that $P = 100000\,Pa$ , $r = 3.44\times 10^{23}$ , $N_{A} = 6.022\times 10^{23}$ , $T = 273.15\,K$ and $R_{u} = 8.314\times 10^{3}\,\frac{L\cdot Pa}{mol\cdot K}$ , then the volume of carbon dioxide at STP is:

$V = \frac{r\cdot R_{u}\cdot T}{N_{A}\cdot P}$

$V = \frac{(3.44\times 10^{23})\cdot \left(8.314\times 10^{3}\,\frac{L\cdot Pa}{mol\cdot K} \right)\cdot (273.15\,K)}{(6.022\times 10^{23})\cdot (100000\,Pa)}$

$V = 12.972\,L$

Therefore, the correct answer is C.

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3 years ago

What mass of hydrogen is produced when 192 g of magnesium is reacted with hydrochloric acid?​

What mass of hydrogen is produced when 192 g of magnesium is reacted with hydrochloric acid?