The energy needed to ionize an atom of si when it is in the most stable is 786.4 kJ mol^-1 however if an atom of Si is in certain low lying excited state only 310.8 is needed to ionize.
what is the wavelength of he radiation emitted when an atom of si undergoes a transition from this excited state to the ground state?

The wavelength of he radiation emitted is

Explanation:

We know that energy needed is given by

 ----- (1)

h = 6.62 × J s

c = 3  ×

E = 786.4 - 310.8 = 475.6

Total energy

E = 78.9 × J

From equation (1)

×

Therefore the wavelength of he radiation emitted is

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"

am i too late?

explanation: