Question
Asked Nov 5, 2019
2. For a mass of 0.010 g Mg and 5.0 mL of 1.00 M HCl, calculate the theoretical partial pressure of
the resulting H2(g) in a flask with V = 145 mL at 25°C
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2. For a mass of 0.010 g Mg and 5.0 mL of 1.00 M HCl, calculate the theoretical partial pressure of the resulting H2(g) in a flask with V = 145 mL at 25°C

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Expert Answer

Step 1

The chemical reaction is as follows,

Mg + 2HClMgCl, +H
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Mg + 2HClMgCl, +H

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Step 2

The moles of Mg and HCl are c...

0.010g
= 0.0004114 mol
Mg Moles
24.305 g/mol
5.0
HCl moles
0.005 moles
1.00x 10 L
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0.010g = 0.0004114 mol Mg Moles 24.305 g/mol 5.0 HCl moles 0.005 moles 1.00x 10 L

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