During bad storage of cement the alkalis in the cement react with CO2 to form alkali carbonates, which they react with Ca(OH)2 liberated by the hydrolysis of --------- to form --- C3S, CaCO3 Calcium Carbonate, C3S Dicalcium silicate, CaCO3
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- Like heavy water (D₂O), so-called “semi-heavy water”(HDO) undergoes H/D exchange. The scenes below depict aninitial mixture of HDO and H₂ reaching equlibrium.(a) Write the balanced equation for the reaction. (b) Is the valueof Kgreater or less than 1? (c) If each molecule depicted repre-sents 0.10 M, calculate K.Subterranean brines in parts of the United States are rich iniodides and bromides and serve as an industrial source of theseelements. In one recovery method, the brines are evaporated todryness and then melted and electrolyzed. Which halogen ismore likely to form from this treatment? Why?formation of X- (aq) assume all atoms used are moatomic solids in the standard state
- What is the balanced equation for water is driven from copper sulfate pentahydtate,CuS04*5H2O,with heat?Write a balanced equation for each of the followingreactions: (a) Burning magnesium metal in a carbondioxide atmosphere reduces the CO2 to carbon. (b) Inphotosynthesis, solar energy is used to produce glucose(C6H12O6) and O2 from carbon dioxide and water.(c) When carbonate salts dissolve in water, they producebasic solutions.21) By decomposition of 50g CaCOa the amount of Cao produced will be - O a) 5.6g O b) 16.8g O c) 28g O d) 56g
- What volume of hydrogen gas forms at SATP when 0.85 g of magnesium metal reacts with excess HCl solution?8. A 2.856-g sample of limestone was analyzed for Fe, Ca, and Mg. The iron was determined as Fe;Os, yielding 0.04561 g. Calcium was isolated as CaSO4, yielding a precipitate of 1.487 g, and Mg was isolated as 0.1599 g of Mg;P2O7. Report the amount of Fe, Ca, and Mg in the limestone sample as %w/w FeO, %w/w CaO, and %w/w MgO.Aqueous solutions of phosphoricacid and potassium hydroxidereact to produce aqueouspotassium dihydrogen phosphateand liquid water. Balance the chemical equation.
- What are theconsequences of shifting thechemical equilibrium of theformation of bicarbonate fromcarbon dioxide and watertowards the consumption ofproducts of the reversereaction?(a) In 20 or less of yourown words define the term “leachate”and describe how it forms. (b) Previous records had shown that to prevent acute toxicity to organisms, the maximum mass of CdSO4 that should be allowed into the landfill was determined to be 0.1 kg. This was calculated using a standard concentration of Cd in mg/L where the volume of the leachate pond was used as 500 000L. (i) Provide the name of the CdSO4 compound. State the oxidation number of Cd in this compound (ii) You need to ensure that the concentration used to determine the mass of Cd allowed in the landfill, meets the current regulatory standard. Assuming that previous calculations determined that all of the CdSO4 would be deposited in the leachate pond, what standard concentration of Cd in mg/L was used to determine the maximum mass of allowable CdSO4?A 600.0 mg sample consisting of only CaC2O4and Mg C2O4is heated at 500oC converting the two salts to CaCO3and MgCO3. The sample weighs 465.0 mg. If the sample had been heated at 900oC where the products are CaO and MgO, what would the mixture of oxides weigh? Write in a padpaper and show the clear and complete solution