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8_murik_8 [283]
3 years ago
14

The bond enthalpy of the C―N bond in the amide group of proteins can be treated as an average of C―N (276 kJ/mol) and C═N (615 k

J/mol) bonds. Calculate the maximum wavelength of light needed to break the amide bond.
Chemistry
1 answer:
Paraphin [41]3 years ago
6 0

Answer:

268 nm

Explanation:

First' let's calculate the average bond energy:

(276 + 615)/2 = 445.5 kJ/mol

By Avogadro's number 1 mol = 6.02x10²³ molecule, then the energy necessary to break the amide bond in 1 molecule is:

E = 445.5/6.02x10²³ = 7.4x10⁻²² kJ = 7.4x10⁻¹⁹ J

So, the wavelength of light (λ) can be calculated by:

E= h*c/λ

Where h is the Planck's constant (6.626x10⁻³⁴ J.s), and c is the light speed (3.0x10⁸ m/s).

7.4x10⁻¹⁹ = 6.626x10⁻³⁴ * 3.0x10⁸/λ

λ = 2.68x10⁻⁷ m

λ = 268 nm

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A large balloon is initially filled to a volume of 25.0 L at 353 K and a pressure of 2575 mm Hg. What volume of gas will the bal
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Answer:

45.0 L is the volume of gas will the balloon contain at 1.35 atm and 253 K.

Explanation:

Using Ideal gas equation for same mole of gas as

\frac {{P_1}\times {V_1}}{T_1}=\frac {{P_2}\times {V_2}}{T_2}

Given ,  

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Also, P (atm) = P (mm Hg) / 760

P₁ = 2575 / 760 atm = 3.39 atm

P₂ = 1.35 atm

T₁ = 353 K

T₂ = 253 K

Using above equation as:

\frac {{P_1}\times {V_1}}{T_1}=\frac {{P_2}\times {V_2}}{T_2}

\frac{{3.39}\times {25.0}}{353}=\frac{{1.35}\times {V_2}}{253}

\frac{1.35V_2}{253}=\frac{3.39\times \:25}{353}

Solving for V₂ , we get:

<u>V₂ = 45.0 L</u>

45.0 L is the volume of gas will the balloon contain at 1.35 atm and 253 K.

4 0
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Oxidation can be defined as the process in which the oxidation number of a substance increases.

On the left side of the equation, Cl has a charge of -1 (in HCl); while on the right side of the equation Cl has a charge of 0 in Cl₂.

Thus, Cl⁻ was oxidized.

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The accepted value for the molar volume of a gas is 22.4 L. Sarah's experimental data indicated that a mole of a gas had a volum
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Answer:

Percent error = 12.5%

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Replacing:

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