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A 4.50-g sample of LIL at 25.oC dissolves in 25.0 mL of water also at 25.0C. The final equilibrium temperature of the resulting solution is 60.8C. What is the enthalp of solution of LICL expressed in kilojoules per mole?
A 29.0-g sample of water at 260. K is mixed with 51.0 g water at 340. K. Calculate the final temperature of the mixture assuming no heat loss to the surroundings.
How many moles of PbI2 are formed? What is the concentration of KNO3? What is the remaining concentration of the reactant that was in excess?
1) Why is it important to clean up any spills immediately, wash hands frequently, and wash glassware thoroughly when working with crystal violet solutions?
what spontaneous reaction will occur in aqueous solution among the ions Sn4+, Sn2+, Co3+, and Co2+ ? What will be the E°cell for this reaction?
Standard Temperature Pressure and Volume, The respiratory rate of a person is 20 breathes per minute. If every average breath is about 310cm^3 of air at 22C and 740mmHG
Which statement is true concerning the reaction... N(g) + N(g) = N2(g) + energy?
Find the mass of sodium required to produce 5.68 L ofo hydrogen gas at STP from the reaction described by the following equation: 2Na+2H2O-->2NaOH+H2
Bottled propane is used in areas away from natural gas pipelines for cooking and heating, and is also the source of heat in most gas barbecue grills. Propane burns in oxygen according to the following balanced chemical equation.
A piece of sodium metal reacts completely with water as follows. 2 Na(s) + 2 H2O(l) ->2 NaOH(aq) + H2(g) The hydrogen gas generated is collected over water at 25.0°C. The volume of the gas is 295 mL measured at 1.00 atm.
Determine the value of the equilibrium constant at this temperature - Ammonium Hydrosulfide NH4HS yields NH3(Ammonia) and Hydrogen sulfide
sulfate dissolves as follows: Na2SO4(s) → 2Na+(aq) + SO42- (aq). How many moles of Na2SO4 are required to make 1.0 L of solution in which the Na concentration is 0.10 M?
A testing facility found that 8.35*10^23 molecules of carbon dioxide were produced when a sample of octane was burned in air. If this combustion process is known to produce an 86.7% yield, how many grams of octane were in the sample?
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