4.The annual production of sulfur dioxide from burning coal and fossil fuels, auto exhaust, and other sources is about 26 million tons. The equation for the reaction isS(s) + O2(g) → SO2How much sulfur (in tons), present in the original materials, would result in that quantity of SO2? (5 points) (g) 5.Each copper(II) sulfate unit is associated with five water molecules in crystalline opper(II) sulfate pentahydrate (CuSO4⋅5H2O). When this compound is heated in air above 100oC, it loses the water molecules are also its blue color:CuSO4⋅5H2O → CuSO4+ 5H2If 9.60 g of CuSO4 are left after heating 15.01 g of the blue compound, calculate the number of moles of water originally present in the compound. (5 points) O 6.The fertilizer ammonium sulfate [(NH4)2SO4] is prepared by the reaction between ammonia (NH3) and sulfuric acid:2 NH3(g) + H2SO4(aq)→ (NH4)2SO4(aqHow many kilograms of NH3are needed to produce 1.00 × 105kg of (NH4)2SO4?(5 points) ) 2 Copyright © 2017 by Thomas Edison State University . All rights reserved.
You've reached the end of your free preview.
Want to read all 5 pages?
- Fall '15
- Stoichiometry, Sulfuric acid, Thomas Edison State University