Question

a 6.017 gram sample of cobalt is heated in the presence of excess sulfur. a metal sulfide is formed with a mass of 9.291 g. determine the empirical formula of the metal sulfide. enter the elements in the order co, s empirical formula =

Explanation:

Step1: Calculate mass of sulfur

Mass of sulfur = Mass of metal - Mass of cobalt. Mass of cobalt is 6.017 g and mass of metal sulfide is 9.291 g. So mass of sulfur $m_S=9.291 - 6.017=3.274$ g.

Step2: Calculate moles of cobalt

Molar - mass of Co is approximately 58.93 g/mol. Moles of Co, $n_{Co}=\frac{6.017}{58.93}\approx0.1021$ mol.

Step3: Calculate moles of sulfur

Molar - mass of S is approximately 32.07 g/mol. Moles of S, $n_S=\frac{3.274}{32.07}\approx0.1021$ mol.

Step4: Determine the ratio of Co to S

The ratio of moles of Co to moles of S is $\frac{n_{Co}}{n_S}=\frac{0.1021}{0.1021}=1:1$.

Answer:

CoS