Question

A 1.000-g sample of lead shot reacted with oxygen to give 1.077 g of product. Fill-in the blanks, to finally determine the empirical formula of the lead oxide. Refer to Example Exercise 1 Record your numbers to 3 significant figures. Do not use exponential notation or subscripts in your answers. a) The mass of oxygen used in the reaction is b) The number of moles of lead is moles and the number of moles of oxygen is moles. c) Using their ratio of number of moles, this yields an empirical formula of

Answer 1

The empertical formula of lead oxide is pro Calculation Step-1 To find the mass of orygen that Meacted is = mass of product - mass of lead = 1:0779 - 1.000 = 0.077 9 ştep-2 To find the mole of each reactant moles = mass/-m-otax-mass- The motan mass of fb = 207 g/mot and of oxygen = 168 /mol moles of lead (pb) = 1.0009 207 gt mot _-_0.004-8_moles moles of teact oxygen = 0.0779 16 g1 not 1000048 moles Step-s. To find the mole ratio gt is devide each mole by smallest numbe ole Co.0048) pb = 0.0048/0.0048 = 1 0 = 0.0048/0.0048= Therefove-empirical formutaris - pro Thanks Your like hall great value fome.. A7 Value