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In a coffee-cup calorimeter, 1.50 g of NH4NO3 is mixed with 76.0 g of water at an initial temperature of 25.00°C. After dissolution of the salt, the final temperature of the calorimeter contents is 23.65°C. Assuming the solution has a heat capacity of 4.18 J/°C · g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.
What is the osmotic pressure of a homogenous solution at the temperature At 25 o C, as this solution is consisting of 21.0 g urea
What is the percent by mass of sulfur trioxide (SO3) if oleum is expressed as 3H2SO4 . 5SO3?
How much 0.230M KOH is required to completely neutralize 55.0mL of 0.220M HClO4
In an experiment, equal volumes of 0.00200M FeCl3 and 0.00200M NaSCN were mixed together and reacted according to the equation:
At 295 K, Keq = 7.0 x 10-2 for the following equilibrium: NH4HS(s) ? NH3(g) + H2S(g) What is the equilibrium partial pressure (in atm) of H2S.
If iron is oxidized to Fe2+ by a copper(II) sulfate solution, and 0.704 grams of iron and 12.6 mL of 0.581M copper(II) sulfate react to form as much product as possible,
C2H4 + 3O2 = 2CO2 + 2H2O If you start with 54 grams of ethylene (C2H4) how many grams of carbon dioxide will be produced?
It decomposes into its elements. Write the balanced equation for this reaction. If 71.8 g of Hgo is decomposed, calculate the volume of oxygen at STP
6Na+Fe2O3->3Na2O+ 2Fe. If you are provided 20.0 moles of sodium & excess iron (III) oxide, how many moles of iron would form?
A 59.0-g sample of an alloy at 93.0°C is placed into 264 g of water at 22.0°C in an insulated coffee cup. Assume that no heat is absorbed by the cup.
Explain Why a glacial Acetic acid in a conductance set-up does forms gradually brighter lights that is dim to bright because it is frequently diluted with water?
An aqueous solution is 22.0% by mass ethanol, CH3CH2OH, and has a density of 0.966 g/mL. what is molality of ethanol
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