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3kg of H2O is boiling at constant temperature 140C. The mass fraction of liquid phase of the substance is 60%. What are the pressure, mass density, internal energy and enthalpy of the entire system?
The boiling point of a solution containing 10.44 g of an unknown nonelectrolyte in 50.00 g of acetic acid is 159.2°C. What is the molar mass of the solute?
When calcium carbonate is added to hydrochloric acid, calcium chloride, carbon dioxide, and water are produced. How many grams of calcium chloride will be produced when 27.0 g of calcium carbonate are combined
A 1.90 g sample of a large boimolecule was dissolved in 11.0 g of carbon tetrachloride. The boiling point of this solution was determined to be 77.85°C. Calculate the molar mass of the biomolecule
A 680 MW coal fired power plant is 34% efficient at producing electricity. The coal has a heating value of 20,000 kJ/kg, an ash content of 5.5% and a sulfur content of 4.5%. Note: 1 MW = 1000 kW , and 1 kW = 1 kJ/s. a. What is the daily input rate..
Important information about Heat of Reaction, The combustion of butane produces heat according to the equation 2C4H10(g) + 13O2(g) --> 8CO2(g) + 10H2O(l) deltaHrxn= -5314kJ
A rigid container of O2 has a pressure of 340 kPa at a temperature of 713 K. What is the pressure at 273 K?
HClO is a weak acid (Ka = 4.0 × 10-8) and so the salt NaClO acts as a weak base. What is the pH of a solution that is 0.087 M in NaClO?
A 0.1000M solution of ethanoic acid (HC2H3O2) is only partially ionized so that [H+]=2.25X10^-3M. What is the acid dissociation constant for this acid?
Polyisobutylene (PIB) is equilibrated in propane vapor at 35 oC. At this temperature, the saturated pressure (p10) of propane is 9050 mm Hg and its density is 0.490 g/cm3
an area of 1.15 m^2 and given that the acceleration due to gravity is 9.8 m/s^2, what is the mass of this column?
Calculate the molar concentration of H3PO4 in this solution: Calculate the number of grams of this solution required to hold 87.5 g H3PO4:
What are some reasons why there would be a difference between the expected and actual values for the moles of copper oxide produced from heating copper in the air.
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