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A 1.500-g sample of gasoline was burned in a bomb calorimeter whose total heat capacity is 13.20 KJ/oC. The temperature of the calorimeter increased from 23.00oC to 27.50oC. (a) What is the experimental heat of combustion of kerosene? (b) If the true value of heat of combustion of kerosene is 43.00 KJ/g what is the percent error?
One gram of H₂O at -50 ⁰C was heated and become 110 ⁰C. Cp ice = 0.5 cal/g-K, Cp steam = 0.48 cal/g-K
At what temperature in degC involved the latent of vaporization?
How much heat in J was involved from the start up to right before melting?
How much heat in J was involved from right upon melting to right before boiling?
How much heat in J was involved from right before boiling up to the end of heating?
Calculate the nuclear binding energy (in joules) and the binding energy per nucleon of the following isotopes:
4 2 He (4.0026 amu)
184 74 W (183.9510 amu)
209 83 Bi (208.9804 amu)
Use this format:
ΔE per nucleon = _____ x 10^_____ J/nucleon
Answers must be in scientific notation.
Using The Particle In a box model, the energy of the Highest occupied for a linear polyene of length 14 and contain 10 electron
1. What is the value of ΔE in a system wherein a car engine that releases heat pushing the piston, doing 451 J of work and losing 325 J to the surroundings?
2. What is the specific heat of a metal whose mass is 94.5 g if the temperature changes from 250°C to 48°C when it absorbs 850 J of heat?
3. A 4.4-g compound is burned in a bomb calorimeter whose total heat capacity is 7.854 kJ/°C. A temperature change of 7.13°C occurred. What is the heat of combustion per gram of the compound?
A 26.3 g sample of Aluminum is heated to 39.2 C then is placed in a calorimeter containing 45.0 g of water. Temperature of water increases from 20.00 C to 22.00 C. What is the specific heat of Aluminum?
https://vaavada.bitbucket.io/
For the reaction shown, find the limiting reactant for each of the following initial amounts of reactants.
2Al(s)+3Cl
2
(g)→2AlCl
3
(s)
39. Approximately two-thirds of all the sulfuric acid
produced for industry is used in the production of
fertilizers. Ammonium sulfate and potassium sulfate
are both fertilizers that are manufactured using
sulfuric acid. At a large fertilizer manufacturing plant,
a technician begins to prepare some tests using a
standard solution of sulfuric acid.
a. The technician measures out 2.50 L of a standard
solution of sulfuric acid with a concentration
of 10.0 mol/L. Determine the amount of water
that must be added to create a solution with a
concentration of 3.75 mol/L.
b. A large beaker contains 655 mL of a standard
solution of sulfuric acid with a concentration of
10.0 mol/L. This beaker is placed in a fume hood
where evaporation can occur. Determine the
amount of water that would have to evaporate in
order for the solution to have a concentration of
11.0 mol/L.
38. Sulfuric acid is used to make chlorine dioxide
for bleaching in the pulp and paper industry. A
technician in a pulp mill needs to make 275 L of a
solution containing 4.25 mol/L of sulfuric acid.
a. Calculate the volume of concentrated sulfuric
acid (17.8 mol/L) that the technician must
measure to make the required solution.
b. Determine the volume of water needed to make
the required solution.
