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Hoochie [10]
3 years ago
15

Calculate the energy required to ionize a ground state hydrogen atom. Report your answer in kilojoules. Socratic.Org

Chemistry
1 answer:
sveticcg [70]3 years ago
7 0
<h3>Answer:</h3>

           ΔE  =  2.18 × 10⁻²¹ kJ

<h3>Solution:</h3>

Using Bohr Energy Equation,

                                    ΔE  =  - R (1/nₐ² - 1/nₓ²)

Where;

           R  =  Rydberg's constant  =  2.18 × 10⁻¹⁸ J

           nₐ  =  Infinity  =  ∞   (electron removed from H atom)

           nₓ  =  1   (Ground state of H atom)

Putting Values in equation 1,

                                    ΔE  =  - 2.18 × 10⁻¹⁸ J × ( 1/∞² - 1/1²)

                                    ΔE  =  - 2.18 × 10⁻¹⁸ J × ( 0 - 1)

                                    ΔE  =  - 2.18 × 10⁻¹⁸ J × (-1)

                                    ΔE  =  2.18 × 10⁻¹⁸ J

                                    ΔE  = 2.18 × 10⁻²¹ kJ

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6 0
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A gas mixture being used to simulate the atmosphere of another planet at 23°c consists of 337 mg of methane, 148 mg of argon, an
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The total pressure of the mixture is 65.5 kPa.

According to Dalton's Law of Partial Pressure,

The partial pressure of gas = Mole fraction of gas × Total pressure

Total Pressure = Sum of all the gases partial pressures

The number of moles of methane is,

Moles \:  of \: methane  \: (16 g/mol) =  337 \: mg  \times  \frac{1 g}{1000 mg} \times  \frac{ 1 mol}{16 g }

= 0.021 mols

The moles of methane are 0.021 mols.

The number of moles of the argon,

Moles \:  of \: argon (40 g/mol) = 148 \:  mg  \times  \frac{  1 g}{1000 mg } \times  \frac{  1 mol}{40 g}

= 0.003 mols

The number of moles of argon is 0.003 mols.

The number of moles of nitrogen is,

Moles  \: of \: nitrogen (28 g/mol) = 296 \:  mg  \times  \frac{ 1 g}{1000 mg}  \times  \frac{  1 mol/}{28 g}

= 0.010 mols

The number of moles of nitrogen is 0.010 mols.

The total number of moles is,

= 0.021 + 0.003 + 0.010

= 0.034 mols

Mole \:  fraction =  \frac{ Moles \:  of \:  solute }{Total \:  number  \: of  \:  moles  \: of  \: soulte \:  and \:  solvent}

= \frac{  0.010 }{ 0.034}

= 0.29

0.29 \: P _{total} = 19 \:  kPa

P _{total} =  \frac{ 19  \: kPa }{0.29}

= 65.5 kPa

Therefore, the total pressure of the mixture is 65.5 kPa.

To know more about Dalton's law, refer to the below link:

brainly.com/question/14119417

#SPJ4

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