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4 years ago

Consider hydrogen atom in an excited state of 3s1. What is the energy of its electron

Chemistry

1 answer:

SVEN [57.7K]4 years ago

8 0

Given:

Excited state electron configuration of H atom = 3s¹

To determine:

Energy of the electron in this state

Explanation:

The energy 'E' of an electron in a hydrogen atom occupying a level, 'n' is given by the formula:

En = -E₀/n²

where, E₀ is the ground state energy = 13.6 eV

n = principle quantum number i.e. n = 1,2,3...

Therefore,

En = -13.6/n² eV

In this case for a 3s¹ configuration, n = 3

E = -13.6/(3)² = -1.51 eV

Ans: Energy of the electron in a 3s1 state is -1.51 eV

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A container of oxygen with a volume of 60 L is heated from 300 K to 400 k, What is the new volume?

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Answer:

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Explanation:

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V2 = V1 T2/T1

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V2 = ?

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3 years ago

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Answer:

For a: The standard Gibbs free energy of the reaction is -347.4 kJ

For b: The standard Gibbs free energy of the reaction is 746.91 kJ

Explanation:

Relationship between standard Gibbs free energy and standard electrode potential follows:

$\Delta G^o=-nFE^o_{cell}$ ............(1)

For a:

The given chemical equation follows:

$2Ce^{4+}(aq.)+3I^{-}(aq.)\rightarrow 2Ce^{3+}(aq.)+I_3^-(aq.)$

Oxidation half reaction: $Ce^{4+}(aq.)\rightarrow Ce^{3+}(aq.)+e^-$ ( × 2)

Reduction half reaction: $3I^_(aq.)+2e^-\rightarrow I_3^-(aq.)$

We are given:

$n=2\\E^o_{cell}=+1.08V\\F=96500$

Putting values in equation 1, we get:

$\Delta G^o=-2\times 96500\times (+1.80)=-347,400J=-347.4kJ$

Hence, the standard Gibbs free energy of the reaction is -347.4 kJ

For b:

The given chemical equation follows:

$6Fe^{3+}(aq.)+2Cr^{3+}+7H_2O(l)(aq.)\rightarrow 6Fe^{2+}(aq.)+Cr_2O_7^{2-}(aq.)+14H^+(aq.)$

Oxidation half reaction: $Fe^{3+}(aq.)\rightarrow Fe^{2+}(aq.)+e^-$ ( × 6)

Reduction half reaction: $2Cr^{2+}(aq.)+7H_2O(l)+6e^-\rightarrow Cr_2O_7^{2-}(aq.)+14H^+(aq.)$

We are given:

$n=6\\E^o_{cell}=-1.29V\\F=96500$

Putting values in equation 1, we get:

$\Delta G^o=-6\times 96500\times (-1.29)=746,910J=746.91kJ$

Hence, the standard Gibbs free energy of the reaction is 746.91 kJ

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