Magnesium metal (0.100 mol) and a volume of aqueous hydrochloric acid that contains 0.500 mol of hcl are combined and react to completion. how many liters of hydrogen gas, measured at stp, are produced? mg(s) + 2hcl(aq) → mgcl2 (aq) + h2 (g)

2.24 L of hydrogen gas, measured at STP, are produced.

Explanation:

Given, Moles of magnesium metal, = 0.100 mol

Moles of hydrochloric acid, = 0.500 mol

According to the reaction shown below:-

1 mole of Mg reacts with 2 moles of

0.100 mol of Mg reacts with 2*0.100 mol of

Moles of must react = 0.200 mol

Available moles of = 0.500 moles

Limiting reagent is the one which is present in small amount. Thus, is limiting reagent.

The formation of the product is governed by the limiting reagent. So,

1 mole of on reaction forms 1 mole of

0.100 mole of on reaction forms 0.100 mole of

Mole of = 0.100 mol

At STP,  

Pressure = 1 atm  

Temperature = 273.15 K

Volume = ?

Using ideal gas equation as:

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.

water and alcohols have similar properties because water molecules contain hydroxyl groups that can form hydrogen bonds with other water molecules and with alcohol molecules, and likewise alcohol molecules can form hydrogen bonds with other alcohol molecules as well as with water.