College Chemistry

Test Preparation AP Test Preparation
1

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<p>It takes 210.5 kJ of energy to remove 1 mole of electrons from 1 mole of atoms on the surface of rubidium metal. How much energy does it take to remove a single electron from an atom on the surface of solid rubidium? Write the answer in J.</p>

<p>What is the maximum wavelength of light capable of doing this in nm?</p>

2

<p>It’s just a conversion:</p>

<p>Divide 208.4 kJ by Avogadros number (6.02x10^23) and multiply by 1000 to convert to Joules.</p>

<p>Then, for the second part, use this formula:</p>

<p>Energy = hc/lamda </p>

<p>where, h = Planck’s constant (6.626x10^-34 J/s)
c = speed of light (3.0x10^8 m/s)
and lamda is the wavelength.</p>