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nordsb [41]
3 years ago
5

2Cl(g) ⇌ Cl2(g)

Chemistry
1 answer:
Nataly [62]3 years ago
6 0

Answer:

-121.301 kJ·mol⁻¹;  57.8 J·K⁻¹mol⁻¹; 464.9 J·K⁻¹mol⁻¹; spontaneous

Explanation:

                         2Cl(g) ⇌ Cl₂(g)

ΔHf°/kJ·mol⁻¹:  121.301       0

S°/J·K⁻¹mol⁻¹:  165.190   223.0

1. ΔᵣH

ΔᵣH = products -reactants = 0 - 121.301 = -121.301 kJ·mol⁻¹

2. ΔᵣS

ΔᵣS = products - reactants = 223.0 - 165.190 = 57.8 J·K⁻¹mol⁻¹

3. ΔS(univ)

\begin{array}{rcl}\Delta S_{\text{univ}} &=& \Delta S_{\text{sys}}  +\Delta S_{\text{surr}}\\\\ &=& \Delta S_{\text{sys}}  -\dfrac{\Delta H_{\text{sys}}}{T}\\\\& = & 57.8 - \dfrac{-121301}{298}\\\\& = & 57.8 + 407.1\\& = & \mathbf{464.9 \,\, J\cdot K^{-1}mol^{-1}}\\\end{array}

4. Spontaneity

\begin{array}{rcl}\Delta G &=& \Delta H - T\Delta S\\& = & -121.301 - 298 \times 0.0578\\& = & -121.301 - 17.23\\& = &  \textbf{-138.5 kJ}\cdot\textbf{mol}^{\mathbf{-1}}\\\end{array}

ΔG is negative, so the reaction is spontaneous.

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The question is incomplete. Complete question is attached below.
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Reason:
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3. They have the same number of electron shells.


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3 years ago
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Explanation:

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6 0
3 years ago
In a reaction vessel, 17.6 g of solid chromium(III) oxide, Cr2O3, was allowed to react with excess carbon tetrachloride in the f
notsponge [240]

Answer:

72.53% is the yield of CrCl3

Explanation:

Given

Reaction:

Cr2O3(s) + 3 CCl4(l) → 2 CrCl3(s) + 3 COCl2(aq)

CCl4 is in excess and 17.6g  Cr2O3 present

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To Find:

% yields of the reaction

Also given

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By the stoichiometry of the reaction

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0r

1 x1 52 g of Cr2O3 gives 2x 158.35 g of CrCl3

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= 36.67 g CrCl3

but actual yield is only 26.6g

so % yield is (26.6 ÷÷ 36.67) × 100

= 72.53% is the yield of CrCl3

8 0
3 years ago
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