Question

Heat of Reaction for the Combustion of Magnesium Although you will not be working with actual chemicals during this laboratory, since you will be doing it virtually, the procedure is given in order for you to be aware of the process that would be followed in a laboratory setting. Introduction In this experiment, you will use Hess's Law to determine the heat for a reaction that is difficult to measure directly. Magnesium metal burns rapidly, releasing light and heat, as observed in photo flashbulbs or by burning magnesium ribbon. The reaction is presented by the equation: Mos + 10269 → Mgos) This equation can be obtained by combining equations (2), (3) and (4): Mgos) + 2HCl(aq) MgClacaq + H200 (2) MS + 2HCl(aq) MgCl2caq) + H269) (3) Hace + 7029) > H,00 (4) By combining these three equations, you can obtain equation (1). The heats of reaction for equations (2) and (3) can easily be determined by experiments. The heat of reaction for equation (4) can be obtained from a table of values for previously measured reactions.

I need the solution for the volume of HCl.

Answer 1

H₂O1 Myis) O molar mass 40 Solo Equation + Mydis + 2HQ Moldy + Equation 3 → +zHC Hd Myll2 + H2(g) given mass of mg Os) (W) = 0.969: w 0196 noi of molex of mgo = 0'024 mass of My(s) = 0.55g., molex of mg = 0.55 24 =0.023 From equation : (2) & (2) , we can say that 2 moles of He is reg. to consume 1 mol. My Oo and I mel. my (5) seperatly. :. mole's of Helfaqi) from eq? (2) 2X 0.024 = 0.048 male & moles of Helag) from eqh (3) = 2X0:023 0.046 mole 7 hence, wt. af HClicq.)(W), from eg" (2-) = 0.0 48x36.5) 1.759 - fwts of HCl(aq) (bz), from egh (3) = (0.0 46X36-5) = 1.689 ( density of HClay. = 118 sme) consider hence vom of Hel in eqh (2) = = 1.48 ml. 1.75 1.18 À voth of Hy in eqh (3) = 1.68 1.42 ml. 1.18