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Be sure to answer all parts. In a future hydrogen-fuel economy, the cheapest source of H2 will certainly be water. It takes 467 kJ to produce 1 mol of H atoms from water. What is the frequency, wavelength, and minimum energy of a photon that can free an H atom from water? Enter your answers in scientific notation. Frequency = 7.05 × 10 -32 s−1 Wavelength = 4.26 × 10 -25 m Minimum energy = × 10 kJ/photon

User Gruff
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1 Answer

4 votes

Answer:


7.7549* 10{19}\ J


1.17037* 10^(15)\ Hz


2.56329* 10^(-7)\ m

Step-by-step explanation:

c = Speed of light =
3* 10^8\ m/s


N_A = Avogadro's number =
6.022* 10^(23)


\\u = Frequency


\lambda = Wavelength

The minimum energy is given by


E=(1\ mol)/(N_A)\\\Rightarrow E=467* 10^(3)* (1)/(6.022* 10^(23))\\\Rightarrow E=7.7549* 10{19}\ J

The minimum energy is
7.7549* 10{19}\ J

The energy of a photon is given by


E=h\\u\\\Rightarrow \\u=(E)/(h)\\\Rightarrow \\u=(467* 10^(3)(1)/(6.022* 10^(23)))/(6.626* 10^(-34))\\\Rightarrow \\u=1.17037* 10^(15)\ Hz

The frequency of the photon is
1.17037* 10^(15)\ Hz

Wavelength is given by


\lambda=(c)/(\\u)\\\Rightarrow \lambda=(3* 10^8)/(1.17037* 10^(15))\\\Rightarrow \lambda=2.56329* 10^(-7)\ m

The wavelength is
2.56329* 10^(-7)\ m

User Rhino
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