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For a particular liquid, raising its temperature from 330 K to 353 K causes its vapor pressure to double. What is the enthalpy of vaporization of this liquid? (R = 8.31 J/(K· mol)) Answer 135 kJ/mol 245 kJ/mol 28.6 kJ/mol 2.41 kJ/mol 286 kJ/mol
The decomposition of N2O to N2 and O2 is a first- order reaction. At 730°C the half-life of the reaction is 3.58 3 103 min. If the initial pressure of N2O is 2.10 atm at 730°C, calculate the total gas pressure after one half-life.
Calculate both the molar and molal concentration of water (H2O) in a solution of pure water when the water is at 10C and 30C. Use an accurate molecular weight for water
The normal boiling point of ethanol is 78.4 C, and the heat of vaporization is Delta H vap = 38.6 kJ / mol.
Determine hydroxyl and hydrogen ion concentration in this solution. (if Ka for ammonium ion = 5.0 x 10^-10.)
This solution was back-titrated with a 0.0440 M Ga3 solution until all the EDTA reacted, requiring 14.0 mL of the Ga3 solution. What was the original concentration of the V3 solution?
When 10.0 g of NH3 reacts, the actual yield of N2 is 8.50 g. What is the percent yield?
What is the total pressure, in mm Hg, of a gas mixture containing argon gas at 0.25 atm, helium gas at 350 mm Hg, and nitrogen gas at 360 torr
petit discovered the empirical rule that the specific heat times the atomic weight of many solid elements is a constant: Using this rule, calculate the specific heat of copper and platinum.
Calculate, in sequence each of the following quantities in the acqueous solution to determine the equilibrium constant for the reaction: a) mole of FeNCS+2 the form in the reacting equilibrium
Calculte w and delta E for the vaporization of 1.00 mol water at 100 degrees celsius and 1.00 atm pressure.
Identify the two important classes of catalysts. Analyze the chemical reactions that take place when a biological catalyst combines with a reactant (substrate) to form an unstable intermediate.
at 900 k the following reaction has kp 0.345.2 so2g o2g 2 so3gin an equilibrium mixture the partial pressures of so2
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