1. Consider the following reaction: 2Hg (l) + O2 (g) 2HgO (s) H = -180 kJ a. Is

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Question

1. Consider the following reaction: 2Hg (l) + O2 (g) 2HgO (s) H = -180 kJ

a. Is the reaction exothermic or endothermic?

b. Calculate the quantity of heat produced/required when 50.0 g of HgO(s) is formed according to this reaction.

c. Is work done on the system, the surroundings, or is no work done for this reaction?

d. How many liters of oxygen gas at 25oC and 1 atm pressure are required to produce 50.0 g of HgO (s) in the presence of excess Hg (l)?

Hello, I was wondering if I could have help on b and d

Since deltaH = -ve , the reaction is exothermic reaction.

From the balanced equation,

Formation of 2 mol of HgO (OR) 2 * 216.6 g. of HgO produces 180 kJ of heat

Then, formation of 50.0 g. of HgO produces 50.0 * 180 / 216.6 = - 41.6 kJ of heat

(c)

Work is done on the system as the volume of the system decreases.

( Because no gaseous substances at products side )

(d) Moles of HgO = mass / molar mass = 50.0 / 216.6 = 0.231 mol

From the balanced equation,

formation of 2 mol of HgO requires 1 mol of O2

then, 0.231 mol of HgO requires 1 * 0.231 / 2 = 0.1155 mol of O2 gas.

Ideal gas equation,

P V = n R T
V = 0.1155 * 0.0821 * 298.15 / 1.00

V = 2.83 L

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