Question

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(11) oxide (Hgo) into liquid mercury and gaseous dioxygen. 2 HgOG) - 2Hg() + O2(g) x 5 ? 2. Suppose 61.0 mL of dioxygen gas are produced by this reaction, at a temperature of 100.0 °C and pressure of exactly 1 am, Calculate the mass of mercury(II)oxide that must have reacted. Round your answer to 3 significant digits. 08

Answer 1

Sal) from the balanced reaction, 249 0(s) → 2Hg (1) + O2(g) Using ideal gas equation for oxygen gas PV=nRT where P = Pressure of gas = 1 ahm V = Volume of gas in La 610 mL = 61.0 x 10-3 L n = moles of gas R= Gas constant = 0.08215 L-ahm malik me = 100°C = 100 +273 = 373K molik T= Absolute Substillate the values, (1.00 alm)x (610x10 -32) = nx0:08215 Lahm X (373K) &n=0.002 moks molar mass of HgO = 216.59 glmal man of HgO= 0.002 moly O₂ x 2 moles Figo X/216-59 g to 1 moloth Imottigo =(0.866 g HgO