Question

oregaseous reactant The great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 1775. In this experiment Lavoisier found that mercury(II)oxide, when heated, decomposed into liquid mercury and an invisible and previously unknown substance: oxygen gas. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(II)oxide (HgO) into liquid mercury and gaseous dioxygen x 5 ? 2. Suppose 51.0 mL of dioxygen gas are produced by this reaction, a temperature of 50.0 °C and pressure of exactly I atm. Calculate the mass of mercury(II)oxide that must have reacted. Be sure your answer has the correct number of significant digits. 0
plesse answer part two.

Answer 1

Solution of problem and formula used shown in the following Image

1. Balanced chemical equation 2 HgO(5) s 2 Hg (1) + O2(g) 2 first calculate moles of Oz produced by using Lideal gas equation. PV = nRT where P = Pressure in atm = 1 atm. v = volume in liter = 0.051 L (1 ml=0.ool litee then siml= 51%0.0015010SIL) In = no. of moles = ? R = gas constant = 0.08206 Liatm molik IT = temperature in Kelvin = 323.15 K. (sol = 273.15 +50% = 323.15 K) we can write above equation In = PUIRT substitute value In = 1 x 0.051/0.082064 323.15 = 0.001923245 moles 102 produced = 0.001923245 moles According to balanced reaction a mole Hgo produce ! mole Og. mola & ratio between Hgo to og is 29) therefore to produce 00001923245 mole og required Hgo = 0.001923245X2 = 0.00384649 mole Hao molae mass of Ago = 26.59 g/mol gm of compound = No. of moles x molat mass gm of HgO = 0.003814649 X 216:59 =0:833111269 om Mass of mercury (11) oxide reacted = 0.83311126g oml Ans= mass of mercury(II)oxide reached = 0.833 am