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When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 14.4 g of carbon were burned in the presence of 50.6 g of oxygen, 12.2 g of oxygen remained unreacted. What mass of carbon dioxide was produced?
Distilled water in equilibrium with air contais dissolved carbon dioxide at a concentration of 1.0 x 10^-5 M. Calculate the pH of such a solution.
Compare the proposed reaction mechanism for the sodiumhypochlorite oxidation of cyclohexanol with that involved in thechromic acid oxidation. Do you notice any similarities?
A mutant hemoglobin has His146 of the beta chain replaced with a threonine residue. predict what the consequence of this mutation might be. specifically:
Manufacturing overhead equal $5, $2, and $3respectively. Calculate the amount of material cost, labor cost, andoverhead cost in the beginning Work in Process.
A 13.74 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 20.49 grams of CO2 and 6.291 grams of H2O are produced.
Describe how the pseudo rate constant, k', is determined from the experimental data? Also describe how k, the true rate constant, is determined from the experimental data
A vat contains 2.29 M sulfuric acid solution. How many kg of KOH will be required to react completely with (neutralize) 882 L of the solution?
a flask that can withstand an internal pressure of 2500 torr, but no more, is filled with a gas at 21.O C and 780 torr and heated. At what temperature will it burst?
How many grams of Mg(NO3)2 (Mm=147 g/mol) must be added to 405 g of water to make a solution with a colligative molality of 0.125 m?
The car has a city mileage of 20 miles per gallon. If the car is replaced with the new car with city mileage off 32 miles per gallon and the average cost of gasoline is $3.62 per gallon, estimate the amount of fuel, energy, and money conserved wit..
525mL of 1.50M NaCl is added to a beaker containing 378mL of 2.22M AgNO3, resulting in the formation of AgCl precipitate.
Determine the number of moles of oxygen that would be needed to completely combust 0.0350 moles of benzene
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