A chemist decomposes samples of several compounds; the masses of their constituent elements are shown. Calculate the empirical formula for each compound. 0.672 g Co, 0.569 g As, 0.486 g O

Combustion analysis of naphthalene, a hydrocarbon used in mothballs, produced 8.80 g CO2 and 1.44 g H2O. Calculate the empirical formula for naphthalene.

A 3.000 g sample of a gaseous compound was found to contain 2.560 g of carbon and 0.440 g of hydrogen. A) What is the simplest formula of the compound (Write C first and then H)? You won't be able to make the numbers a subscript. For instance, for MgCl2 enter MgCl2. B) The molar mass of the compound was found to be 42.08 g/mol. What is the molecular formula of the compound? You won't be able to make the numbers a subscript. For instance, for MgCl2 enter MgCl2.

D. Calculate the mass (g) of the following samples. 25) 238 moles of lead 26) 1.54 x 10⁹ moles of Zn 27) 7.70 x 10-⁹ moles of Mg(NO3)2 28) 8.42 x 1027 atoms of tin 29) 6.39 x 10¹8 atoms of sulfur 30) 5.99 x 1030 molecules of SiO₂

Combustion analysis of 1.200 g of an unknown compound containing carbon, hydrogen, and oxygen produced 2.086 g of CO2 and 1.134 g of H2O. What is the empirical formula of the compound?Combustion analysis of 1.200 g of an unknown compound containing carbon, hydrogen, and oxygen produced 2.086 g of CO2 and 1.134 g of H2O. What is the empirical formula of the compound?C2H5OC3H8O2C2H5O2C2H10O3

The class of ternary compounds called carboranes (containing the elements carbon, boron and hydrogen) have played a prominent role in many areas of fundamental chemical research. In particular, they have provided many interesting examples for testing theories on chemical bonding and structure. A particular carborane has the following mass percentages: 21.30%C and 67.09%B. What is the empirical formula of this compound? Choose appropriate coefficients in the formula below. C B H

1:  Find the empirical formula for a compound that is 34.59% NA, 23.31% P, and 42.10% O by mass?  2: find the empirical formula for a sample of which contains 0.388 g LI, 2.992g Cr, and 3.147g O?

A chemist decomposes samples of several compounds; the masses of their constituent elements are listed. Calculate the empirical formula for each compound. Express your answer as a chemical formula   0.2907 g F, 0.1224 g O 0.524 g Na, 0.569 g As, 0.486 g O  1.443 g Se, 2.591 g Cl