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Five kg of water initially a saturated vapor at 100kPa are cooled to saturated liquid while the pressure is maintained constant. Sketch the process on a p-v diagram. Determine the work and heat transfer for the process each in kJ.
A 1- flask is filled with 1.20 g of argon at 25 C. A sample of ethane vapor is added to the same flask until the total pressure is 1.25 atm.
A gas mixture being used to simulate the atmosphere of another planet consists of 319 mg of methane, 171 mg of argon, and 212 mg of nitrogen
A 58.0 mL solution of 0.500 M Cd(NO3)2 is prepared. What mass of NaOH is needed to precipitate the Cd2+ ions from this solution?
What is the movement of electrons in an ammonia and hydrochloric acid reaction?
Nitrogen and hydrogen combine at high temperature, in the presence of a catalyst, to produce ammonia. N2(g) + 3H2(g) --> 2NH3(g) Assume 0.170 mol of N2 and 0.543 mol of H2 are present Initially
Calculate the temperature of the system once equilibrium has been reached. Assume that Cp,m for Au and H2O is constant at its value for 298K throughout the temperature range of interest.
Calculate the molar solubility of AgBr in a 1.00 M aqueous solution of ammonia. Then calculate the solubility of AgBr in pure water, and compare the two solubilities. (Ksp for silver bromide is 7.7x10 -13 and Kf for Ag(NH3)2+ is 1.6x10^7)
a solution is prepared by adding enough water to 387 g of CsCl to form 1 liter of solution. What is the mass of the solution? the density of the solution is 1.384 g/mL.
Calculate standard Delta G for the following reaction at 25 C. You will have to look up the thermodynamic
Energy cost of dissociation was found to be 4 kWh/m3 of CO2. Calculate conversion degree of CO2 into CO and O2 in this system.
Arrange these compounds in order of increasing boiling point and explain your reasoning. (assume similar mass) CH3OCH3 CH3CH2CH3 CH3CH2OH 2. Which of the following compounds would have the greater viscosity?
Calculate the value of the reaction quotient Q. (b) Is the system at equilibrium? If not, predict which way (right or left) the reaction will proceed to reach equilibrium.
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