Respuesta :
Answer:
2.24 L of hydrogen gas, measured at STP, are produced.
Explanation:
Given, Moles of magnesium metal, [tex]Mg[/tex] = 0.100 mol
Moles of hydrochloric acid, [tex]HCl[/tex] = 0.500 mol
According to the reaction shown below:-
[tex]Mg_{(s)} + 2HCl_{(aq)}\rightarrow MgCl_2_{(aq)} + H_2_{(g)}[/tex]
1 mole of Mg reacts with 2 moles of [tex]HCl[/tex]
0.100 mol of Mg reacts with 2*0.100 mol of [tex]HCl[/tex]
Moles of [tex]HCl[/tex] must react = 0.200 mol
Available moles of [tex]HCl[/tex] = 0.500 moles
Limiting reagent is the one which is present in small amount. Thus, [tex]Mg[/tex] is limiting reagent.
The formation of the product is governed by the limiting reagent. So,
1 mole of [tex]Mg[/tex] on reaction forms 1 mole of [tex]H_2[/tex]
0.100 mole of [tex]Mg[/tex] on reaction forms 0.100 mole of [tex]H_2[/tex]
Mole of [tex]H_2[/tex] = 0.100 mol
At STP,
Pressure = 1 atm
Temperature = 273.15 K
Volume = ?
Using ideal gas equation as:
[tex]PV=nRT[/tex]
where,
P is the pressure
V is the volume
n is the number of moles
T is the temperature
R is Gas constant having value = 0.0821 L.atm/K.mol
Applying the equation as:
1 atm × V L = 0.100 × 0.0821 L.atm/K.mol × 273.15 K
⇒V = 2.24 L
2.24 L of hydrogen gas, measured at STP, are produced.
