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3 years ago

Calculate the mass of 2.50 mol of CH,OH(1). Show your work. Use the appropriate

Chemistry

1 answer:

Sophie [7]3 years ago

7 0

Answer:

80.1 grams

Explanation:

Find the molar mass of CH3OH first by using the periodic table values.

12.011 g/mol C + (1.008*3 g/mol H) + 15.999g/mol O + 1.008 g/mol H

=32.042 so that is the molar mass

Now that you have 2.50 moles of CH3OH, you can calculate the mass in g

2.50molCH3OH * (32.042g CH3OH / 1 mol CH3OH) = 80.105

32.042g / 1 mol is the same as 32.042 g/mol

Since there are 3 sig figs in the problem (2.50 has 3 sig figs), you round to 80.1 g CH3OH

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If you hit the surface of Iron with a photon of energy and find that the ejected electron has a wavelength of .75 nm, what is th

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Explanation:

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$KE = h\frac{c}{\lambda_{p}} - \phi$ (1)

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KE: is the kinetic energy of the electron

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c: is the speed of light = 3.00x10⁸ m/s

$\lambda_{p}$ : is the wavelength of the photon =?

Φ: is the work function of the surface (Iron) = 4.5 eV

The kinetic energy of the electron is given by:

$KE = \frac{p^{2}}{2m} = \frac{(\frac{h}{\lambda_{e}})^{2}}{2m}$ (2)

Where:

p: is the linear momentum = h/λ

m: is the electron's mass = 9.1x10⁻³¹ kg

$\lambda_{e}$ : is the wavelength of the electron = 0.75 nm = 0.75x10⁻⁹ m

Hence, the wavelength of the photon is:

$\frac{(\frac{h}{\lambda_{e}})^{2}}{2m} = h\frac{c}{\lambda_{p}} - \phi$

$\lambda_{p} = \frac{hc}{\frac{h^{2}}{2m\lambda_{e}^{2}} + \phi} = \frac{6.62 \cdot 10^{-34} J.s*3.00\cdot 10^{8} m/s}{\frac{(6.62 \cdot 10^{-34} J.s)^{2}}{2*9.1 \cdot 10^{-31} kg*(0.75 \cdot 10^{-9} m)^{2}} + 4.5 eV*\frac{1.602 \cdot 10^{-19} J}{1 eV}} = 1.728 \cdot 10^{-7} m = 172.8 nm$

Therefore, the wavelength of the incoming photon is 172.8 nm.

I hope it helps you!

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3 years ago