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Calculate w (in kJ) when 566 g iron (III) oxide (MM = 159.7 g/mol) reacts with excess carbon to produce carbon dioxide gas at 332 K: 2Fe2O3(s) + 3C(s) ? 4Fe(s) + 3CO2(g)
the concentration of co2 in the soda is 0.14M. find the concentration of CO2 in the soda after the bottle is opened, and equilibrates at a partial pressure of 3.0 X 10^-4 atm. The henry's law constant is 3.4 X 10^-2 mol/L atm.
When most Fe^3+ salts are dissolved in dilute nitric acid, the solution is often yellow to orange-yellow in color. Why could you not visually detect these colors in Fe(NO3)3 stock solution
Sulfuric acid,H2SO4 is a strong diprotic acid. A sample of aqueous solution of sulfuric acid has a concentration of 0.0582 M. Calculate the concentration of H3O+ ion, HSO4- and (SO4)2- ions from this solution. Ka = 1.18 * 10^-2
Equal volumes of cold 4.184M NaOH at 20C and warm 4.184M HCl at 77.3C are mixed together in a highly efficient calorimeter. what is the final temperature of the solution
A solution containing .2g of an unknown substance in 2.5 g of cyclohexane is found to freeze at 5.1 C what is the molar mass of the unknown substance
The solubility of cerium sulfate, Ce2(SO4)3, in water is 0.34 g per 100 mL at 100 °C and 14.2 g per 100 mL at 10 °C. Is the dissolving of cerium sulfate in water an endothermic or exothermic process
How long must a current of 0.75 A pass through a sulfuric acid solution in order to liberate 0.100 L of H2 gas at STP
What will be the effect on your final %carbonate if a drop of HCl is spilled, and is not delivered to the test tube? Explain reasoning.
Experimental write up without changing our kinetics calculation. Write the structure of another other organic products that might be produced from the carbocation intermediate in this reaction.
Calculate the molarity of 464 mL of a solution that contains 135 g of sucrose C12H22O11
A solution is prepared by mixing 250 mL of 1.00 M CH3COOH with 500 mL of 1.00 M NaCH3COO.
A 0.9157g mixtureof CaBr2 and NaBr is dissolved in water and AgNO3 is added to the solution to form AgBr Precipitate. If the mass of the precipitate is 1.6930g, what is the percent by mass of NaBr in the original mixture
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