A constant amount of metal (Mg) about 0.080 g is reacted with two acids (HCl and H2SO4) to produce hydrogen gas a. write out a correctly formatted hypothesis that describes how the amount of hydrogen gas produced will be affected by the concentration of acid. b. write out a correctly formatted hypothesis that describes how the amount of hydrogen gas produced will be affected by the type of acid (HCl or H2SO4) reacted with the Mg metal

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Asked Nov 14, 2019
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A constant amount of metal (Mg) about 0.080 g is reacted with two acids (HCl and H2SO4) to produce hydrogen gas 

a. write out a correctly formatted hypothesis that describes how the amount of hydrogen gas produced will be affected by the concentration of acid. 

b. write out a correctly formatted hypothesis that describes how the amount of hydrogen gas produced will be affected by the type of acid (HCl or H2SO4) reacted with the Mg metal 

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Expert Answer

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Step 1

Metal reacts with a solution of an acid to produce a soluble or insoluble salt and hydrogen gas (H2). According to the collision theory, the increase in the concentration of reactants increases the frequency of collisions which in turn increases the number of products. The increase in the concentration of acid increases the number of hydrogen ions in the solution. So, the amount of hydrogen gas increases on increasing the concentration of acid.

Step 2

The reaction of magnesium with HCl and H2SO...

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Mg(s)+2HC1(ag)-»MgCl, (aq) H2 (g) Mg(s)HSO (a)»MgSO,(aq)+H2 (g)

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