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scoundrel [369]
1 year ago
5

If a hydrogen atom has its electron in the n = 3 state, how much energy in ev is needed to ionize it?

Chemistry
1 answer:
tensa zangetsu [6.8K]1 year ago
4 0

The energy of the hydrogen atom will be -0.85 ev.

Ionization, also known as ionization, would be the phenomenon by which an atom or molecule gains or loses electrons to acquire a negative and positive charge, frequently in conjunction with those other chemical changes. Ions are the name for the electrically charged molecular or atom that results.

These chemicals are known as ionic compounds, with table salt serving as an example. Ionization would be the process of removing electrons from such an element as well as a molecule as well as the dissociation of an ionic material, such as salt, itself into the individual ions in a solution like water.

The energy of hydrogen atom will be calculated by using the formula:

E_{n} = -13.6 ev / n^{2}

where, E_{n} = energy of nth level, n is the state.

It is given that, n = 3 .

Now put the value of n in above equation.

E_{4} = -13.6 ev / 4^{2}\\E_{4} = -13.6 ev  / 16\\E_{4} = -0.85 ev

Therefore, the energy of the hydrogen atom will be -0.85 ev.

To know more about energy

brainly.com/question/1932868

#SPJ4

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Original molarity was 1.7 moles of NaCl

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Given Information:

Original (concentrated) solution: 25 g NaCl in a 250 mL solution, solve for molarity

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1. Solve for the molarity of the original (concentrated) solution.

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Molarity (M) = 0.43 mol NaCl solute / 0.250 L solution = 1.7 M NaCl (original solution)

2. Solve for the molarity of the final (diluted) solution.

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Answer:

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Explanation:

It seems the question is incomplete. However, this problem has been found in a web search, with values as follow:

" A certain substance X melts at a temperature of -9.9 °C. But if a 350 g sample of X is prepared with 31.8 g of urea (CH₄N₂O) dissolved in it, the sample is found to have a melting point of -13.2°C instead. Calculate the molal freezing point depression constant of X. Round your answer to 2 significant digits. "

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So now we have all the required data to <u>solve for Kf</u>:

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