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Consider an ice cube weighing 18g initially at T=0 C transderred into a well-insulated container at T=20 C and P= 1 bar that had about 24 L of air. The whole system reaches equilibrium in the end. You may assume that the container does not allow for heat exchange with the surroundings (heat excahnge between ice and air inside container is allowed) The heat of fusion of water is (delta)H fus= 6021 J/mole at 0 C and heat capacity of water liquid is 4.18 J/ (K x g)
a) Assume the total heat capacity of the air C air=30 J/K. Describe what's the likely ice will ne after the system reaches equilibrium.
b) Estimate theliekly final temperature after reaching equilibrium
c) How much ice will be melted? How much ice will remain?
How many resonance structures are there for the cyclohepatrienyl cation? Draw them. Are carbon-carbon bonds equivalent?
A gas measures 180. ml. at 870C and 800. mm Hg. Find its volume at standard temperature and 800 mm Hg of pressure.
You are a hazmat responder and walk into what appears to be a meth lab. There are flasks of iodine, White Gas fuel, Sodium Hydroxide, Nitric Acid, and a box of ephidrine.
When 0.060 mol of propionic acid, C2H5CO2H, is dissolved in 500 ml of water, the equilibrium concentration of H3O+ ions is measured to be 2.41 x 10-3 M. What is Ka for this acid?
A 1.996 gram sample of unknown monoprotic acid is dissolved in some water. This acid solution is then titrated to the end point with 27.38 mL of a solution of 0.4165 M KOH.
If 159 of wet is collected over water at 24 and a barometric pressure of 739 , how many grams of have been consumed? (The vapor pressure of water is 22.38 .)
Determine the molar mass of the nonelectrolyte if the osmotic pressure of the solution = 23.6 atm, also express your answerin g/mol?
A mixture of CaCO3 and CaO weighing 0.635 g was heated to produce gaseous CO2. After heating, the remaining solid weighed 0.427 g. Assuming all the CaCO3 broke down to CaO and CO2,
What is the chemical formula of a homonuclear diatomic gas if it has a pressure of 1.40 atm and a density of 1.82 g/L at 27 ºC?
Given that Iron(III) oxide or ferric oxide (molar mass = 159.7 g/mol) reacts with Carbon monoxide (molar mass = 28.0 g/mol).
What are the equilibrium partial pressures? Nitrogen dioxide decomposes according to the reaction given below where Kp = 4.48 x10^-13
Determine the molar concentration of chloride ions after adding 225 ml of 0.625 MKCL with 615 ml of 0.385M MgCl2 if final volume of the solution is 840ml.
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