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A certain sample of coal contains 1.60 percent sulfur by mass. When the coal is burned, the sulfur is converted to sulfur dioxide. To prevent air pollution, this sulfur dioxide is treated with calcium oxide (Cao) to form calcium sulfite (CaSO3). Calculate the daily mass (in kilograms) of CaO needed by a power plant that uses 5.60 * 106 kg of coal per day. Enter your answer in scientific notation. x 10 kg of Cao

One of the reactions that occurs in a blast furnace, in which iron ore is converted to cast iron, is Fe2O3 + 3C0 - 2Fe + 3C02 a Suppose that 1.19 x 103 kg of Fe is obtained from a 1.90 x 10kg/sample of Fe,O3. Assuming that the reaction goes to completion, what is the percent purity of Fe2O3 in the original sample? ]% purity

Ammonia is produced by the reaction of nitrogen and hydrogen according to the equation N269) + 3H2(g) - 2NH3(9) Calculate the mass of ammonia produced when 34.0 g of nitrogen react with 13.2 g of hydrogen. g NH3 Which is the excess reactant and how much of it will be left over when the reaction is complete? O hydrogen o nitrogen 8

Diethyl ether is produced from ethanol according to the following equation: 2CH3CH2OH() - CH3CH2OCH2CH3(1) + H2O(1) 1 Calculate the percent yield if 54.7 g of ethanol reacts to produce 13.1 g of ether. 58.6 x yield

The interhalogen compound CIF, reacts with NH2 to produce three products according to the figure shown here: N H a F If 27.3 g of NH3 and 168.2 g of ClFz are allowed to react, what masses of each product would be recovered assuming complete reaction? | 8 N₂ g Cl2 g HF