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The mass of a hydrated CaSO4• X H2O sample is 3.08 g. After heated gently for 20 min, the mass of the sample reduces to 2.72 g (water is completed removed by heating and only CaSO4 is left). How many H2O (X) are in CaSO4• X H2O?
a bicycle tire is filled with air to a pressure of 100 psi at a temperature of 100 degrees c. riding the bike on
What is a balanced equation to represent the formation of the precipitate formed between silver and chloride
An excess of O2 reacted with 3.68 g of Fe. What is the percent yield if 4.86 g of Fe2O3 are isolated
A system receives 93 J of electrical work, performs 227 J of pressure-volume work and releases 155J of heat.What is the change in Internal energy of the system?
vessel above eqm is established and at eqm, partial pressure of SO3 and SO2 are same, calculate no. of moles of O2 present at eqm
How much dry solute would you take to prepare each of the following solutions from the dry solute and the solvent?
calculate the PH of a solution made by adding 5.00gram of sodium hydride,NaH,to enough water to make 0.900 litre of solution?
Draw a schematic of the flow. Clearly define and label the axes and any variables to be used. Indicate on the schematic the fluid on top and bottom of the slit.
What is the average current passing through a solution of NiSO4 if 1.25 g of Ni were deposited in 4.07 hours? i = A
How does this affect the reported solubility product of borax at that temperature? Explain. Temperatures can range from 4.4 degrees C, 17.1 degrees C, 34.6 degrees C, 41.6 degrees C, and 50.6 degrees C.
Calculate the change in temperature that occurs when 4.55 g of solid NaOH is added to 100.0 g of water in a constant pressure calorimeter. The specific heat of the solution
Sulfur has two solid forms - a (or rhombic) and b (or monoclinic). The standard enthalpies of combustion, in which the product is SO2, are -296.53 kJ/mol for S(s,a) and -296.86 kJ/mol for S(s,b). Find the standard reaction enthalpy for the process..
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