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The answer to formula and calculationsurvey of physical chemistry
State all of the assumptions (e.g. ideal gas etc).
(previous reaction is 2H??2(g) + O2(g) ----> 2H2O(g))
Given the reaction in the previous questionat 298 Kelvin where H2 has a partial pressure of 0.10 bar, O2 is at 0.20 bar, and H2o is at 1.5 bar:(a) Determine the direction and quantify the change in free energy the reaction must undergo to reach equilibrium.
(b) Calculate the equilibrium constant.
(c) Illustrate the reaction on a plot of Free Energy versus % Reactants/Products (show ?GO, the approximate position of Q for the given partial pressures, and the position of Q at equilibrium).
magnesium sulphate MgSO4 has an observed osmotic pressure =7.6 atm at the temperature of twenty five degree celsius. Determine the observed van't Hoff factor?
How will you prepare the following solutions from 6.0 M solutions of acetic acid and ammonia. Give exact details. Assume that a 10-mL graduated cylinder.
A 1.000 g sample of a compound containing C, H and O is burned in excess oxygen, producing 1.783 g CO2 and 0.734 g H2O. Determine the empirical formula of the compound.
A mixture of MgCO3 and MgCO3·3H2O has a mass of 3.057 g. After heating to drive off all the water the mass is 2.790 g. What is the mass percent of MgCO3·3H2O in the mixture.
Explain Net Ionic Equations and Balancing, These are only eight out of a fifty-three question hand out, but with eight answers to reference off of I think I'll be far more successful in my attempts at this.
In a beaker, I mix 50 ml of 3 M HCl with 100 ml distilled water. Both fluids are at 25 C initially. (Cp mix =. 0.985 cal/g-C) a. what is the final T.
The valve between these Tanks X and Y is opened and the gases are permissible to mix. After the gases have had time to mix, calculate the partial pressure of the oxygen gas?
Determine the phase composition and temperature when equilibrium is reestablished?
What mass of sucrose should be combined with 468 of water to make a solution with an osmotic pressure of 8.75 at 295 ? (Assume the density of the solution to be equal to the density of the solvent.)
If 18.5 mL of 0.800 M HCl solution are needed to neutralize 5.00 mL of a household ammonia solution, what is the molar concentration of the ammonia.
Assume that 0.406 mol Carbon (g) is placed in a cylinder that is expanding. The barometric pressure on the outside of the cylinder is constant at 1.00 atm and the temperature is 300.0 K.
What is the volume of the container needed to store 0.8 moles of argon gas at 5.3 atm and 227°C.
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