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Calculate the mass in grams for pure silver sample that loses 3.28 when its temperature drops from 146 to 23 celsius.
The mass percent of a three component gas sample is 58.0% C2H4O2, 14.6% NH3 and 27.4% CH2O. Calculate the partial pressure (atm) of CH2O if the total pressure of the sample is 0.340 atm.
A real gas behaves most nearly like an ideal gas: a. at high pressure and low temperature b. at low pressure and high temperature
Calculate the mass of methane that must be burned to provide enough heat to convert 128.0 g of water at 36.0°C into steam at 103.0°C.
175g of water at 86.0 degrees C were added to a perfect calorimeter conataining 103 grams of water at 18.5 C. What is the final temperature of this water mixture?
If 0.214 mol of argon gas occupies a volume of 652 mL at a particular temperature and pressure, what volume would 0.375 mol of argon occupy under the same conditions?
What is the pH of the solution at the equivalence point for the titration of 100 mL of a .786 M HCO2H solution with a .786 M Solution of sodium Hydroxide? Formic acid has a Ka=1.80*10^-4.
If 3.00 g of (NH4)2SO4 is dissolved in enough water to form 200. mL of solution, what is the molarity of the solution?
When 7.00 moles of gas A and 3.00 moles of gas B are combined, the total pressure exerted by the gas mixture is 1.0 atm. What is the partial pressure exerted by gas A in this mixture?
A flask contains 0.180 mol of liquid bromine. Determine the number of bromine molecules present in the flask
One of the starting substances in smog formation is NO. Assuming that the temperature in a running automobile engine is 1100°C, estimate KP for the above reaction.
Calculate the amount of heat required to completely sublime 33.0 g of solid dry ice CO2 at its sublimation temperature. The heat of sublimation for carbon dioxide is 32.3 kJ/mol.
List all stable isotopes of Xenon and at least 4 unstable ones. Give the decay-channels, their end products and their half-life. (Use no abbreviations).
In one city, a balloon with a volume of 6.0 L is filled with air at 101 kPa pressure. The balloon in then taken to a second city at a much higher altitude. At this second city, atmospheric pressure
What is the molarity of a solution of 12.0 g of NH4Br in enough H2O to make 240 mL of solution?
How many milliliters of 0.0898 M NaOH are required to titrate the 25.00 mL of benzoic acid solution in the flask to the equivalence-point?
What is the normal boiling point in of ethyl alcohol if a solution prepared by dissolving 26.0 of glucose in 285 of ethyl alcohol has a boiling point of 79.1? kb of alcohol is 1.22
Assume that we measure a rate of reaction using zinc with 1.25 M HCl at room temp(20degrees cels.) How much slower or faster will these two chemicals react at 40 degrees celsius?
Calculate the mass of ammonium nitrate that should be heated to obtain 100 mL of dinitrogen oxide, N20, at 1.00 atm and 25 degrees celcius
Several interesting observations from the world around you are listed below. Which of these is NOT explained by a colligative property?
A sample of carbon dioxide occupies at 2.54dm3 container at STP. What is the volume of the gas at a pressure of 4HCL +O2 ---> 2CL + 2H20
In a purity check for industrial diamonds, a 10.00 carat (1 carat = 0.2000 g) diamond is heated to 74.21°C and immersed in 26.05 g of water in a constant-pressure calorimeter. The initial temper
Calculate the quantity in grams of formic acid and sodium formate necessary to make 500 mL of a buffer that has a formic acid concentration of .75 M and a sodium formate concentration of .75 M.
The EPA limit for lead in the water supply is 15 parts per billion by mass. Calculate the number of lead ions present in 1.00 kg of water that is at the EPA limit for lead.
A 1.20 sample of dry ice is added to a 745 mL flask containing nitrogen gas at a temperature of 25.0 C and a pressure of 735mmHg . The dry ice is allowed to sublime (convert from solid to gas) and t