One reaction that produces hydrogen gas can represented by the following unbalanced chemical equation: #Mg(s) + HCl(aq) - MgCl_2(aq) + H_2(g)#. What mass of HCl is consumed by the reaction of 2.50 moles of magnesium?

Question

One reaction that produces hydrogen gas can represented by the following unbalanced chemical equation: #Mg(s) + HCl(aq) -> MgCl_2(aq) + H_2(g)#. What mass of HCl is consumed by the reaction of 2.50 moles of magnesium?

Naomi Aronson · Accepted Answer

Well we need the stoichiometric equation..............and calculate that #182.3*g# of #HCl# are evolved..............

#Mg(s) + 2HCl(aq) rarr MgCl_2(aq) + H_2(g)uarr# And, given #2.5*mol# metal (and stoichiometric acid), CLEARLY, there are #5.0*mol# #HCl# consumed......... And thus mass of #HCl=5.0*molxx36.46*g=182.3*g#.

Jose Ayala · Answer

undefined To find the mass of HCl consumed, you need to use stoichiometry. First, balance the equation: Mg(s) + 2HCl(aq) -> MgCl2(aq) + H2(g). Then, calculate the molar mass of HCl (1.00794 g/mol for H + 35.453 g/mol for Cl). Next, use the balanced equation to find the mole ratio of Mg to HCl (1 mole Mg reacts with 2 moles HCl). Finally, multiply the moles of magnesium (2.50 moles) by the mole ratio and the molar mass of HCl to find the mass of HCl consumed.

One reaction that produces hydrogen gas can represented by the following unbalanced chemical equation: #Mg(s) + HCl(aq) -&gt; MgCl_2(aq) + H_2(g)#. What mass of HCl is consumed by the reaction of 2.50 moles of magnesium?

One reaction that produces hydrogen gas can represented by the following unbalanced chemical equation: #Mg(s) + HCl(aq) -> MgCl_2(aq) + H_2(g)#. What mass of HCl is consumed by the reaction of 2.50 moles of magnesium?