Homework 24
- Page ID
- 28939
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A photon of wavelength 0.787 nm strikes a surface. The surface has a binding energy of 1.35 *1010 10^-19 kJ/mol. What is the kinetic energy of the emitted electron in eV?
Solution
Strategy:
- Convert kJ/mol à J to keep units consistent.
- Solve For energy of the photon
- Subtract binding energy from the energy of the photon
- Convert J --> eV
- 1.35*10^-19 kJ/mol = 1.35*10-16 J/mol
- Energy=(Planck's Constant)(Speed of light)/ wavelength
- h= 6.626* 10^-34 (Planck’s Constant)
- c=2.99*1010 10^-16 m/s (speed of light)
- E=Energy
- wavelength (convert to meters)
- Energy of photon= binding energy + kinetic energy
- 1.67*r10^-16 J=Kinetic energy
- 1.167*10^-16 J* * 1 eV/1.603*10^-19 J
- =728.5 eV
8.37
How many moles of H2 form for each amount of C2H6 reacted?
C2H6 (g) ---> C2H2(g)+2H2(g)
- 2.1 mol C2H6
- mol C2H6 --> mol H2
- 3.4 mol C2H6
- mol C2H6 --> mol H2
- 5.68 g C2H6
- Convert g C2H6--> mol C2H6 ---> mol H2
- 2.35 g C2H6
- Convert g C2H6 --> mol C2H6 --> mol H2
(Hint: In the equation, the number before the molecule is the amount of moles that specific molecule expresses. If it doesn’t have a number, that molecule has 1 mole)
Solution
(Hint: When converting from grams (g) to moles, divide by the number in the denominator (molar mass) to cancel out grams. Use the periodic table.)
1) 2.1 mol C2H6 * 2 Mol H2/ 1 Mol C2H6= 4.2 mol H2
2) 3.4 mol C2H6 * 2 Mol H2/ 1 Mol C2H6= 6.8 mol H2
3) 5.68 g C2H6 *1 Mol C2H6/ 30 Mol C2H6 = .1893 mol C2H6
.1893 mol C2H6 *2 Mol H2/ 1 Mol
4) 2.35 g C2H6*1 Mol C2H6/ 1 Mol C2H6= .0783 mol C2H6
.0783 mol C2H6*2 Mol H2/ 1 Mol C2H6 H2