When coal is burned, the sulfur it contains is converted into sulfur dioxide. Th

Question

When coal is burned, the sulfur it contains is converted into sulfur dioxide. This SO_2 is a serious pollutant, so it needs to be removed before it escapes from the stack of a coal fired plant. One way to remove the SO_2 is to add limestone, which contains calcium carbonate, CaCO_3 to the coal before it is burned. The heat of the burning coal converts the CaCO_3 to calcium oxide, CaO. The calcium oxide reacts with the sulfur dioxide in the following reaction: 2CaO + 2SO_2 + O_2 rightarrow 2CaSO_4 The solid calcium sulfate does not escape from the stack as the gaseous sulfur dioxide would. What mass of calcium sulfate forms for each 1.00 Mg (Megagram) of SO, removed by this technique? A precipitation reaction takes place when a water solution of potassium phosphate, K_3PO_4, is added to a water solution of cobalt(II) chloride, CoCl_2. Write a balanced equation for this reaction.

Explanation / Answer

Q14

mass of CaSO4 forms when

mass = 1*10^6 grams of SO2 is removed

so..

mol of SO2 = mass/MW = (10^6)/32 = 31250 mol of SO2

ratio is 2:2

or 1 mol of CaSO4 per 1 mol of SO2

31250 mol of SO2 = 31250 mol of CaSO4

so

MW of CaSO4 = 136.14

mass = mol*MW = 31250*136.14 = 4254375 grams = 4254375*10^-6 Mg = 4.254375 megagrams

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