A substance in cough drops is composed of C, H, and O. A 0.1005g sample is combusted, producing 0.2829g of CO2 and 0.1159g of H2O. What is the empirical formula?

4.45 If 21 g of H2S is mixed with 38 g of O2 and 31 g of SO2 forms, what is the percentage yield? 2H2S+3O22SO2+2H2O

Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid-fuel rocket motors. The reaction is Fe2O3(s)+2Al(s)2Fe(l)+Al2O3(s) What masses of iron(III) oxide and aluminum must be used to produce 15.0 g iron? What is the maximum mass of aluminum oxide that could be produced?

A large family of boron-hydrogen compounds has the general formula BxHy. One member of this family contains 88.5% B; the remainder is hydrogen. What is its empirical formula?

The iron oxide Fe2O3 reacts with carbon monoxide (CO)to give iron and carbon dioxide: Fe2O3+3CO2Fe+3CO2 The reaction of 433.2 g Fe2O3 with excess CO yields254.3 g iron. Calculate the theoretical yield of iron(assuming complete reaction) and its percentage yield.

Methane (CH4) is the main component of marsh gas. Heating methane in the presence of sulfur produces carbon disulfide and hydrogen sulfide as the only products. a. Write the balanced chemical equation for the reaction of methane and sulfur. b. Calculate the theoretical yield of carbon disulfide when 120. g of methane is reacted with an equal mass of sulfur.

In Example 4.2, you found that a particular mixture of CO and H2 could produce 407 g CH3OH. CO(g) + 2H2(g) CH3OH (l) If only 332 g of CH3OH is actually produced, what is the percent yield of the compound?

Consider the following unbalanced chemical equation for the combustion of pentane (C5H12): C5H12(l)+O2(g)CO2(g)+H2O(l) If 20.4 g of pentane are burned in excess oxygen, what mass of water can be produced, assuming 100% yield?

What mass of compound is present in 5.00 moles of each of the compounds in Exercise 52?

Calcium carbonate forms carbon dioxide and calcium oxide when it is heated above 900 °C in a limekiln. When heated to 1000 °C in a laboratory, 4.31 g calcium carbonate produces 2.40 g calcium oxide and 1.90 g carbon dioxide. Outline a method similar to combustion analysis by which you could determine the empirical formula for calcium carbonate from these data. Carry out the determination.