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The He gas is contained in a one-liter flask that is connected to an empty one-liter flask with a closed stopcock between the two flasks. While the stopcock is opened some of the He enters the evacuated flask. For this system
A. H is positive and S is negative
B. H is zero and S is positive
C. H is zero and S is negative
D. H is negative and S is positive
When 1.543 g of copper(II) sulfate pentahydrate is heated to drive off the water of hydration, how many grams of copper(II) sulfate and water are formed?
A year later a single large crystal of mass 50 g is at the bottom of the flask. Explain how this experiment provides evidence for a dynamic equilibrium between the saturated solution and the undissolved solute.
An electric power station annually burns 3.3 107 kg of coal containing 1.4 percent sulfur by mass. Calculate the volume of SO2 emitted at STP
How many grams of MgO are produced when 40.0 g of O2 react completely with Mg?
A gas is placed in a storage tank at pressure of 30.0 atm at 20.3 degrees Celsius. As a safety device, there is a small metal plug in the tank made of metal alloy that melts at 125 degrees Celsius.
How many grams of riboflavin (molecular mass = 374.6g/mol) are required to prepare a 1.00L solution that is 5.00 x 10^-5 M
Consider the titration of 30.0mL of 0.050M NH3 with 0.025 M HCl. Calculate the pH after the following volumes of tirant have been added.
Determine the pH of each of the following solutions Part A. 8.3x10^-3 M phenol
The solubility of KNO3 is 155g per 100g of water at 75 degree Celsius and 38.0 g at 25 degree Celsius. Explain what mass in grams of KNO3 will crystallize out of solution if exactly 100g of its saturated solution at 75 degree Celsius is cooled to ..
A piece of metal that has a density of 5.2 g/cm3 and a mass of 100 g was placed in a full jar of water. How many mL of water spilled out of the jar?
Calculate the molar mass of the unknown gas. (Remember that the faster the rate of effusion, the shorter the time required for effusion of 1.0 L; that is, rate and time are inversely proportional.)
Cl2(g) + F2(g) 2 ClF(g) Kc = 19.9 For the reaction forming ClF the initial concentrations are as follows: [Cl2] = 0.5 M ; [F2] = 0.2 M ; [ClF] = 7.3 M Is the reaction at equilibrium? If not, in which direction with the reaction shift to reach eq..
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