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You are given the following boiling point data: Which of the liquids would you expect to have the highest vapor pressure at room temperature?
Water, H2O 100oC
Methanol, CH3OH 64.96oC
Ethanol, CH3CH2OH 78.5oC
Diethyl ether, CH3OH2-O-CH2CH3 34.5oC
Ethylene glycol, HO-CH2-CH2-OH 198oC
A 65 L sample of dry air cools from 133°C to -16°C while the pressure is maintained at 2.85 atm. What is the final volume?
What is the enthalpy of formation of CO(g) in kJ. 2CO(g) + O2(g) --> 2CO2(g). H reaction = -566 kJ ; ?H CO2(g) =-393.5 kJ/mol.
When adding the solution of HNO3 from the buret in Step 14 to beaker 4, you know that you added 2.5 mL instead of 1.5 mL for a total volume of 11.0 mL. How would the calculated value of the equilibrium constant be affected for this sample?
Which of the following solutions is a good buffer system? A) A solution that is 0.10 M HF and 0.10 M NaC2H3O2 B) A solution that is 0.10 M NaOH and 0.10 M KOH C) A solution that is 0.10 M HC2H3O2 and 0.10 M NaC2H3O2 D) A solution that is 0.10 M HC..
Calculate the [Zn2+] in a solution of ZnC2O4 held at a pH of 3.00. Remember C2O4^2- is a weak base so you must consider other equilibria.
Calculate the masses of the reactants and products of the following equation. Please show work.
What is the pH of 0.185M sodium phenolate (C6H5ONa), the sodium salt of phenol (Ka= 1.0 X 10-10)
What is the theoretical yield of bismuth when 346 g of Bi2O3 reacts with excess carbon as shown below?
Draw (a) planar conformation and (b) nonplanar (chair) conformation of trans 1,4-dimethylcyclohexane.
How many mL of Br2 (l) with a density of 3.12 g/mL must you dispense to have 1.56 mole (mol) of Br2 (l).
Is 1.39 at 400oC. Suppose that 1.4 mole of P4 (g) and 1.25 mol of P2(g) are mixed in a closed 25.0-L at 400oC. Determine the reaction quotient and the direction of the reaction.
Cesium has the smallest ionization energy of all the elements (376 kJ/mol), and chlorine has the most negative electron affinity (-349 kJ/mol).
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