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How many liters of CH4 (g), measured at 23.4C and 768mmHG, must be burned to provide the heat needed to vaporize 3.78 L of water at 100C? DeltaHcomb= -8.90x10^2 KJ mol CH4. For H2)(l) at 100 C, d= 0.958 g cm and deltaHvap=40.7KJ mol.
What is the molecular weight of a gas if a 31.0 g sample has a pressure of 836 mm Hg at 25.0°C in a 2.00 L flask? (R= 0.0821 L atm/mol K)
The normal boiling point of the liquid is 425 K. Liquid, X, and Y are all in equilibrium at 342 K and 1800 bar. Tc = 571K, Pc= 46 bar
Write the structures of the saytzeff elimination
Europium (Europium is a chemical element with the symbol Eu and atomic number 63 )crystallizes in a body-centered cubic lattice compute the unitcell edge length in pm if The density of Eu is 5.26 g/cm3..
What is the pressure inside a 5.00 L vessel containing 0.0040 mol of nitrogen gas at a temperature of 23 degrees C
experiment to determine delta H of solution, would you expect to get a larger, smaller or identical temperature change? why?
If 2 x 10-4 moles of S2O82- in 50 mL solution are consumed in 188 seconds, what is the rate of consumption of S2O82-
Compute the concentrations of all species in a 0.900 M sodium sulfite solution. If it is given that the ionization constants for H2SO3 are Ka1=1.4x10^-2 and Ka2=6.3x10^-8.
Determine the fraction of N2 molecules traveling between 500 and 600 m/sec at room temperature
Determine what volume of .1 M HBr is required to neutralize 50 ml of .140 M Barium hydroxide and determine the normality of a solution consisting of 10.51 mg of NaOH in 591 mL of solution
In the titration of a solution of a weak monoprotic acid with a .1325M solution of of NaOH, the pH was halfway to the equivalence point was 4.42.
A 52.0-g sample of an alloy at 93.0°C is placed into 379 g of water at 22.0°C in an insulated coffee cup. Assume that no heat is absorbed by the cup.
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