You have a racemic mixture of d-2-butanol and l-2-butanol. the d isomer rotates polarized light by +13.5∘. what is the rotation

Answer:

189.2 KJ

Explanation:

Provided Data

light wavelength = 632.8 nm

Convert nm to meters

1 nm = 1 x 10⁻⁹

632.8 nm = 632.8 x 1 x 10⁻⁹ = 6.328 x 10⁻⁷m

What is the energy of 1 mole of photons?

Solution

Used Formula

                     E = hc/λ

where

E = energy per photon

h = Planck's Constant

Planck's Constant = 6.626 x 10⁻³⁴ Js

c = speed of light

speed of light = 3 × 10⁸ ms⁻¹

λ = wavelength of light

Insert values into the equation

                   E = hc/λ

                   E = 6.626 x 10⁻³⁴ Js ( 3 × 10⁸ ms⁻¹ / 6.328 x 10⁻⁷m)

                   E = 6.626 x 10⁻³⁴ Js (4.741 x 10¹⁴s⁻¹)

                  E = 3.141 x 10⁻¹⁹J

3.141 x 10⁻¹⁹J indicates the energy for a single photon

Next, we need to determine the energy for 1 mole of photons

It is known that

1 mole contains 6.022 x10²³ photons

Consequently,

     Energy for one mole of photons = 3.141 x 10⁻¹⁹J x  6.022 x10²³

     Energy for one mole of photons = 1.89 x 10⁵ J

Now convert J to KJ

1000 J = 1 KJ

1.89 x 10⁵ J = 1.89 x 10⁵ /1000 = 189.2 KJ

Thus,

the energy for one mole of photons is 189.2 KJ

Answer:

The equation formulated by Michaelis-Menten is expressed as

v₀ = Kcat × [E₀] × [S] / (Km + [S])

in which,

Kcat denotes the experimental reaction rate constant; [S] signifies the concentration of the substrate, and

Km represents the Michaelis-Menten constant.

Explanation:

Refer to the attached image for an in-depth clarification

Hello! The mass percent composition of nitrogen in NH₄OH is 14/35×100. To find the percent composition by mass of an element within a chemical compound, divide the atomic mass of that element (AM), which is 14 for Nitrogen, by the entire compound's molar mass (MM) and multiply that by 100. The formula for determining percent composition is as follows: Have a nice day!

a

The visual representation is displayed in the following image.

For calculations, consider 100 grams of the compound:

ω(Cl) = 85.5% ÷ 100%.

ω(Cl) = 0.855; signifying the mass percentage of chlorine in the compound.

m(Cl) = 0.855 · 100 g.

m(Cl) = 85.5 g; this represents the mass of chlorine.

m(C) = 100 g - 85.5 g.

m(C) = 14.5 g; indicating the mass of carbon.

n(Cl) = m(Cl) ÷ M(Cl).

n(Cl) = 85.5 g ÷ 35.45 g/mol.

n(Cl) = 2.41 mol; this is the quantity of chlorine.

n(C) = 14.5 g ÷ 12 g/mol.

n(C) = 1.21 mol; this is the quantity of carbon.

n(Cl): n(C) = 2.41 mol: 1.21 mol = 2: 1.

The compound in question is identified as dichlorocarbene CCl₂.