Question

When active metals such as magnesium are immersed in acid solution, hydrogen gas is evolved

(a) Write the balanced equation (including physical states) for the reaction of magnesium metal with hydrochloric acid.

(b)Calculate the volume of the H2(g) at 30.1C and 0.85 atm that can be formed when 275 mL of 0.725 HCl solution reactions with excess Mg according to the balanced equation.

Answer 1

Ans - @ The balanced equation for the reaction of magnesium metal with hydrochloric acid is Mg(s) + 2 Hellas) mallz (aq) + 32 (9) 6 Ans - Given that Pressure, P = 0.85 atm Temperaturo, T= 30.1°C - 273+30.1k = 303.1k g assumed that the concentration of Hell is 0.725 m. Jince mg is present in exces so , He is the limiting reagent and the product will fermed accordingly. According to balanced equation , 2 mdrs of He produced Imole of the No. of moes of Hell = (275 x 0.725 millimoles of Hel = 199.375 millimoles of Hell .. = 0.199 nous of Hel [ imde 100 mili) : 0.199 modes of Hell will produced 1 x 0.199 modes of the = 0.099 moles of the

We have pv=nRT , U= nRT vure R = 0.0821 Latin mallar Jubstituting the values we get V- 0.299 males y 0.08 21 Lato mo 'k 'x 303.1k 0.85 am 2.464 L 0-85 = 2.8952 This the same of the $19) is 2.8 982 LLAR