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Masteriza [31]
2 years ago
8

Hello people ~

Chemistry
2 answers:
kotykmax [81]2 years ago
7 0

Answer:

separation of amine mixtures

Explanation:

There are three types of amines

  1. Primary(1°)
  2. Secondary (2°)
  3. Tertiary(3°)

Hinsberg approach is used distinguish between these amines

Roman55 [17]2 years ago
3 0
<h3>CHEMISTRY</h3>

Option A. and B.

The Hinsberg test, which can distinguish primary, secondary, and tertiary amines, is based upon sulfonamide formation. In the Hinsberg test, an amine is reacted with benzene sulfonyl chloride. If a product forms, the amine is either a primary or secondary amine, because tertiary amines do not form stable sulfonamides.

#BRAINLYEVERYDAY

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The rate constant for the second-order reaction !s 0. 54 m-1 s-1 at 300°c. how long (in seconds) would 1t take for the concentra
Jlenok [28]

The answer is 3.63. seconds.

Second order reaction is the reaction in which the rate of reaction depends on either the concentration of two reactant species or on the two times the concentration of single reactant species.

What is the integrated rate law for the second-order reaction?

  • The integrated rate law that relates the concentration, time and rate constant for the second-order reaction is:

\frac{1}{[A]} =\frac{1}{[A]_{0} } +kt

Where

\[\begin{array}{l}{\rm{[A]  -  concentration\ of\ reactant\ A\ at\ time\ t}}\\{{\rm{[A]}}_0}{\rm{ -  initial\ concentration\ of\ reactant\ A}}\\{\rm{t - time}}\\{\rm{k  -  rate\ constant}}\end{array}\]

  • Now, in the given question,

k = 0.54 m^{-1}. s^{-1}

[NO_{2} ]= 0.62\ M

[NO_{2} ]_{0} = 0.28\ M

  • Thus, using the rate law, the time is calculated as-

\frac{1}{0.28\ M} =\frac{1}{0.62\ M } +(0.54 m^{-1}.s^{-1})  t\\\\(0.54 m^{-1}.s^{-1})  t= \frac{1}{0.28\ M} -\frac{1}{0.62\ M } = 1.959 \\\\

Therefore,

t =\frac{1.959}{0.54} = 3.63\ seconds

  • Hence, the it would take 3.63 seconds for the concentration of NO_{2} to decrease from 0.62 M to 0.28 M if the reaction is second order.

To learn more about second order reaction visit:

brainly.com/question/17217385

#SPJ4

3 0
2 years ago
A piece of metal with a mass of 23.2 g at 120.1oC is placed in a styrofoam cup containing 35.0 g of water at 22.2oC. Once the sy
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Answer:

0.8797 J/g oC

Explanation:

use mcAT=mcaT

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Atomic theory question Rutherford’s model
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bounce

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Which of the following statements is true about both nuclear fusion and nuclear fission?
creativ13 [48]

The correct answer is A.

B is incorrect because that only applies to nuclear fission.

C is incorrect because it only applies to nuclear fusion.

D is incorrect because energy can be neither created nor destroyed meaning that this statement is physically impossible,

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What is the MOLAR heat of combustion of methane(CH₄) if 64.00g of methane are burned to heat 75.0 ml of water from 25.00°C to 95
melamori03 [73]

Answer:

-5.51 kJ/mol

Explanation:

Step 1: Calculate the heat required to heat the water.

We use the following expression.

Q = c \times m \times \Delta T

where,

  • c: specific heat capacity
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  • ΔT: change in the temperature

The average density of water is 1 g/mL, so 75.0 mL ≅ 75.0 g.

Q = 4.184J/g.\°C \times 75.0g \times (95.00\°C - 25.00\°C) = 2.20 \times 10^{3} J = 2.20 kJ

Step 2: Calculate the heat released by the methane

According to the law of conservation of energy, the sum of the heat released by the combustion of methane (Qc) and the heat absorbed by the water (Qw) is zero

Qc + Qw = 0

Qc = -Qw = -22.0 kJ

Step 3: Calculate the molar heat of combustion of methane.

The molar mass of methane is 16.04 g/mol. We use this data to find the molar heat of combustion of methane, considering that 22.0 kJ are released by the combustion of 64.00 g of methane.

\frac{-22.0kJ}{64.00g} \times \frac{16.04g}{mol} = -5.51 kJ/mol

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