MgCl2(aq)+2HCl(aq) yields MgCl2(aq)+H2(g) a. How many mL of a 6.00M HCl solution are required to...


MgCl2(aq)+2HCl(aq){eq}\rightarrow {/eq}MgCl2(aq)+H2(g)

a. How many mL of a 6.00M HCl solution are required to react with 15.0g magnesium?

a. How many grams of hydrogen gas can form when 0.500L of 2.00M HCl reacts with excess magnesium?

Stoichiometry and Molar Ratios:

The amount of product that can possibly be produced in a reaction, or the quantity of reactant needed to react with another quantity, can be calculated by stoichiometric calculations. Stoichiometric calculations involve using the molar ratios determined using the balanced reaction equation. The balanced reaction equation shows the ratio of formula units between chemicals by using the coefficients. These ratios are persevered when converting to the number of moles because the mole is just a way to count the number of formula units in a sample. Therefore the fist step to begin any stoichiometric calculations is to convert the known quantity of one chemical into the number of moles of that chemical.

Answer and Explanation:

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a. The molar mass of magnesium is 24.305 g/mol. The number of moles of magnesium in 15.0 g is

{eq}n = \frac {15.0 \ g}{24.305 \ g/mol} \\ n = 0.617...

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Learn more about this topic:

Stoichiometry: Calculating Relative Quantities in a Gas or Solution


Chapter 9 / Lesson 4

Learn how to find the molarity of a solution or the moles of gas in a given volume using stoichiometry. See examples of calculating moles from molarity.

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