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2 years ago

Discussion the sn1 and sn2 substitution reactions. Haloalkanese

1 answer:

8 0

The SN₁ substitution reaction, in which the halogen is released from the haloalkane, and the nucleophile attacks the carbon's positive charge. SN₂ in which the nucleophile attacks the halogen's carbon, causing the halogen to be replaced in which nucleophile attack.

<h3>What is substitution reaction?</h3>

Substitution reactions are those reactions in which one functional group is replaced by another functional group.

Two types of substitution reactions can occur in haloalkanes: SN1 and SN2.

Thus, the SN₁ substitution reaction, in which the halogen is released from the haloalkane, and the nucleophile attacks the carbon's positive charge. SN₂ in which the nucleophile attacks the halogen's carbon, causing the halogen to be replaced in which nucleophile attack.

Learn more about substitution reactions

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Calcium and titanium atoms have the same mass

timofeeve [1]

Answer:

these elements do not have the same masses.

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3 years ago

Calculate the number of moles when 3.00l of a gas at 814 mmhg and 25 °c?

Mariulka [41]

Volume=V=3L
Pressure=P=814mmHg
Temp=T=25°C

No of moles=n

$\\ \rm\rightarrowtail PV=nRT$

$\\ \rm\rightarrowtail n=\dfrac{PV}{RT}$

$\\ \rm\rightarrowtail n=\dfrac{814(3)}{25R}$

$\\ \rm\rightarrowtail n=2442/25R$

$\\ \rm\rightarrowtail n=97.7Rmol$

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2 years ago

An unknown gas effuses at one half the speed of oxygen. What is the molar mass of the unknown? It is either HBr or HI. Which gas

sertanlavr [38]

Answer:

HI.

Explanation:

Thomas Graham found that, at a constant temperature and pressure the rates of effusion of various gases are inversely proportional to the square root of their masses.

Rate of effusion ∝ 1/√molar mass.

<em>(Rate of effusion of O₂) / (Rate of effusion of unknown gas) = (√molar mass of unknown gas) / (√molar mass of O₂).</em>

An unknown gas effuses at one half the speed of that of oxygen.

∵ Rate of effusion of unknown gas = 1/2 (Rate of effusion of O₂)

∴ (Rate of effusion of O₂) / (Rate of effusion of unknown gas) = 2.

Molar mass of O₂ = 32.0 g/mol.

∵ (Rate of effusion of O₂) / (Rate of effusion of unknown gas) = (√molar mass of unknown gas) / (√molar mass of O₂).

∴ 2.0 = (√molar mass of unknown gas) / √32.0.

( √molar mass of unknown gas) = 2.0 x √32.0

By squaring the both sides:

∴ molar mass of unknown gas = (2.0 x √32.0)² = 128 g/mol.

∴ The molar mass of sulfur dioxide = 80.91 g/mol and the molar mass of HI = 127.911 g/mol.

<em>So, the unknown gas is HI.</em>

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3 years ago

Student conducts an experiment to determine the enthalpy of solution for lithium chloride dissolved in water. the student combin

nirvana33 [79]

Answer:- $\Delta H_s_o_l_n=-37.2\frac{kJ}{mol}$

Solution:- First of all we calculate the heat absorbed or released when the solute is added to the solvent. Here the solute is LiCl and the solvent is water.

To calculate the heat absorbed or released we use the formula:

$q=ms\Delta T$