When active metals such as magnesium are immersed in acid solution, hydrogen gas is evolved. Calculate the volume of H2(g) at 30.1°C and 0.85 atm that can be formed when 275 mL of 0.725 M HCl solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride, as shown in the reaction below. Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)                        A)    4 × 10–3 L                                 B)    2.2 L                        C)    2.9 L                        D)    5.8 L                        E)    11.7 L

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Asked Dec 6, 2019
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When active metals such as magnesium are immersed in acid solution, hydrogen gas is evolved. Calculate the volume of H2(g) at 30.1°C and 0.85 atm that can be formed when 275 mL of 0.725 M HCl solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride, as shown in the reaction below. 

Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)

                        A)    4 × 103 L        
                        B)    2.2 L
                        C)    2.9 L
                        D)    5.8 L
                        E)    11.7 L

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Expert Answer

Step 1

Number of moles of HCl can be calculated using the given molarity and volume.

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No.of moles Volume(L) Molarity=- No.of moles=Molarity× Volume(L) =0.725M×0.275L =0.199 mol

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Step 2

From the given balanced equation, it can be seen that one mole H2...

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2HCI+Mg > Н, (9)+MgClL, 2molHClproduces →1molH, 0.199 molHC1 produces -> х molн, 0.199 molHCl×1molH, No.of moles of н, 2mol HCl =0.1mol

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