When 2.004 g calcium is heated in pure nitrogen gas, the sample gains .4670 g of nitrogen. Calculate the empirical formula of the resulting compound.

A 4.78 g sample of a compound with the formula CyH,O, is combusted and yields 11.9 g CO2 and 5.86 g H20. What is the empirical formula of the compound?

A 21.57 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 21.09 grams of Co, and 4.317 grams of H20 are produced. In a separate experiment, the molar mass is found to be 90.04 g/mol. Determine the empirical formula and the molecular formula of the organic compound.

Cobalt(II) chloride forms several hydrates with the general formula CoCl2 ·x H2O , where  x  is an integer. If the hydrate is heated, the water can be driven off, leaving pure  CoCl2  behind.   Suppose a sample of a certain hydrate is heated until all the water is removed, and it's found that the mass of the sample decreases by 22.% . Which hydrate is it? That is, what is  x ?

An organic compound contains Carbon, Hydrogen, and Oxygen. The percentages of H is 6.73%, 39.99% C and 53.28 g of O by mass. What is the empirical formula of the compound? HTML Editore BIUA A I E E = 3 E X 田, Vx D VD¶ T

When ammonia is mixed with hydrogen chloride (HCl), the white solid ammonium chloride (NH4Cl) is produced. Suppose 10.0 g ammonia is mixed with the same mass of hydrogen chloride. What substances will be present after the reaction has gone to completion, and what will theirmasses be?

A compound containing chromium, Cr; chlorine, Cl; and oxygen, O, is analyzed and found to be 33.6% chromium, 45.8% chlorine, and 20.6% oxygen by mass. What is the empirical formula of the compound? The molar mass of chromium, Cr, is 51.996 gmol; the molar mass of chlorine, Cl, is 35.45 gmol; and the molar mass of oxygen, O, is 15.999 gmol.