Calculate the enthalpy for this reaction:
2C(s) + H2(g) ---> C2H2(g) ΔH° = ??? kJ
Given the following thermochemical equations:
C2H2(g) + 5⁄2O2(g) ---> 2CO2(g) + H2O(ℓ) ΔH° = -1299.5 kJ
C(s) + O2(g) ---> CO2(g) ΔH° = -393.5 kJ
H2(g) + 1⁄2O2(g) ---> H2O(ℓ) ΔH° = -285.8 kJ
What is 226.2 kJ?
100
solve: 20 + (30 -11) x 42
What is 324?
100
Ultraviolet radiation has a frequency of 6.8 × 1015
1/s. Calculate the energy, in joules, of the
photon.
What is 2.923 x 10-41 ?
100
Equation relating wavelength and frequency
What is (wavelength)(frequency) = speed of light
(Lambda)(v) = c?
200
.25 moles of product are produced in an exothermic reaction. Find the change in enthalpy for the reaction if 1000 J are released. (Assume everything in the reaction has a 1:1 mole ratio)
What is 4000 J/mol or 4 kJ/mol?
200
Calculate the enthalpy of the following chemical reaction:
CS2(ℓ) + 3O2(g) ---> CO2(g) + 2SO2(g)
Given:
C(s) + O2(g) ---> CO2(g) ΔH = -393.5 kJ/mol
S(s) + O2(g) ---> SO2(g) ΔH = -296.8 kJ/mol
C(s) + 2S(s) ---> CS2(ℓ) ΔH = +87.9 kJ/mol
What is -1075 kJ?
200
32(1/16 + 1/4)2
What is 0.195 ?
200
The energy in kJ for an x-ray photon with a frequency of 2.4 × 1018 1/s.
What is 1.59 x 10-15 ?
200
3.00 x 108 m/s
What is the speed of light?
300
.25 moles of product are produced in an exothermic reaction. The change in enthalpy for the reaction is -1000 J/mol. How much energy is released to the surroundings? (Assume everything in the reaction has a 1:1 mole ratio)
What is 250 J?
300
Calculate ΔH for the following reaction:
8 Al(s) + 3 Fe3O4(s) → 4 Al2O3(s) + 9 Fe(s)
Al2O3 ΔH = -1669.8 kJ
Fe3O4 ΔH = -1120.9 kJ
What is ΔH = -3316.5 kJ ?
300
solve for x: 1/(2/5x) = 2/4
What is 0.2 ?
300
The wavelength (in nm) for light with a frequency of 4.74 x 1014 1/s.
What is 633 nm?
300
h = 6.63 x 10-34 J s
What is Planck's constant?
400
1.5 moles of product are produced in an endothermic reaction. Find the change in enthalpy for the reaction if 1200 J are absorbed. (Assume everything in the reaction has a 1:1 mole ratio)
What is 800 J/mol?
400
Calculate ΔH for the ionization of hydrogen bromide:
HBr(g) → H+(aq) + Br-(aq)
ΔH HBr = -36.2 kJ
ΔH Br- = -120.9 kJ
What is ΔH = -84.7 kJ ?
400
solve for x: 6.2 x 108 = 12(1/x + 1/4)
What is 1.94 x 10-8 ?
400
The wavelength for light with a frequency of about 7.5 x 1014 Hz.
What is 400 nm?
400
The rearrangement of v = E/h to solve for wavelength.