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The normal boiling point of Cl2(1) is -34 °C, where its latent heat of vaporization is 20.4 kJ/mol. Its molar mass is 70.91 g/mol. (a) Calculate the internal energy change (deltaU) for vaporization of 100 g of Cl2(liq.) at this temperature and 1 bar? (b) Calculate its molar entropy change (AS) for vaporization at this condition
Determine hydroxyl and hydrogen ion concentration in this solution. (if Ka for ammonium ion = 5.0 x 10^-10.)
Magnesium Hydroxide is a slightly soluble substance. If the pH of a saturated solution of Mg(OH)2 is 10.49 at 25 degrees celcius, calculate Ksp for Mg(OH)2.
Draw the structure of Caffeine. Skeletal form only. Locate 2 bonds in the molecule that are obviously polar covalent.
what would the rate constant be at a temperature of 150C for the same reaction described in Part A?
The net energy EN is just the sum of the two expressions above. Determine (a) the minimum bonding energy, E0, and (b) the equilibrium interionic distance, r0.
A student was given a standard Fe(s) | Fe2+(aq) half-cell and another halfcell containing an unknown metal M immersed in 1 M MNO3(aq).
The density of chloroform, a widely used organic solvent, is 1.4832 at 20 . How many milliliters would you use if you wanted 119.0 of chloroform.
How many grams of water can be cooled from 36 degrees celsius to 23 degrees celsius by the evaporation of 53g of water.
Rutherford result also showed that the most of the atom's mass is located in the nucleus which has a very small volume.
What volume of .2 M Na2SO4 will completely react with 50 mL of .135 M Ba(NO3)2
theoretically feasible in a solution that initially 0.250 M in each ion? c.) If separation is feasibe in eithee (a) or (b), what ranfe of anode potential (vs. SCE) should be used?
A 15.00 mL sample of a 0.100 M solution of lead(II) nitrate is reacted with 10.00 mL of 0.170 M sodium chloride. How many grams of lead(II)
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