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The enthalpy of combustion of benzoic acid (C6H5COOH) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be 3226.7 kj?mol. when 2.9683 g of benzoic acid are burned in a calorimeter, the temperature rises from 21.84 C to 24.67 C. What is the heat capacity of the bomb? (Assume that the quantity of water surrounding the bomb is exactly 2250 g.)
What volume in L is occupied by 19.62 g of methane, CH4 (MM = 16.04 g/mol) at 23 °C and 1.34 atm?
Describe two different ways by which electrons can move from the valence band to the conduction band.
Calculate Keq for 2 moles of electron(s) in each half-reaction and a standard potential of 0.12 V. Calculate Keq for 2 moles of electron(s) in each half-reaction and a standard potential of (-0.54) V.
Calculate the molarity of 464 mL of a solution that contains 135 g of sucrose C12H22O11
Vanillin, the dominant flavoring in vanilla, contains C, H, and O. When 1.05 g of this substance is completely combusted, 2.43 g of CO2 and 0.50 g of H20 are produced. What is the empirical formula of vanillin?
Rank each of the following measurements from smallest to largest
Calculate the empirical formula of the compound (CxHyOz). B) If the 4.00g sample corresponds to 0.0666 moles of a compound, what is the molecular formula of the unknown molecule (CxHyOz)
A standard mixture containing 2.00 ppm and 2.50 ppm gave a Fe / Mn signal ratio (quotient) of 1.05. A 5.00 mL unknown Fe solution was mixed with 1.00 mL solution containing 12.5 ppm Mn
Combustion of 3.00 g of this compound produced 7.06 g of CO2 and 1.93 g of H2O. What is the empirical formula of the unknown compound?
57.0 mL of a 1.80 M solution is diluted to a volume of 238 mL. A 119-mL portion of that solution is diluted using 117 mL of water. What is the final concentration.
Consider the titration of 50.0 mL of 0.217 M hydrazoic acid (HN3) (Ka = 2.6 x 10-5) with 0.183 M NaOH. determine the pH of the solution before any NaOH is added ?
Assuming that the calorimeter absorbs only a negligible quantity of heat and that the density of the final solution is 1.0 g/mL, calculate the enthalpy change per mole of BaSO4 formed.
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