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3 years ago

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The decomposition of nitryl chloride is described by the following chemical equation: 2NO2C1(g) → 2NO2 (g)-C12 (g) Suppose a two

-step mechanism is proposed for this reaction, beginning with this elementary reaction NO, Cl(g)→NO2(g)+Cl(g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism.

1 answer:

Gnoma [55]3 years ago

6 0

Answer:

Second reaction

NO2 + F -------> NO2F

Rate of reaction:

k1 [NO2] [F2]

Explanation:

NO2 + F2 -----> NO2F + F slow step1

NO2 + F -------> NO2F fast. Step 2

Since the first step is the slowest step, it is the rate determining step of the reaction

Hence:

rate = k1 [NO2] [F2]

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What is empirical and moleculer formula?.

den301095 [7]

The molecular formula shows the exact number of molecules. Therefor, the empirical formula is the simplest formula of the molecular formula

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3 years ago

Ham radio operators often broadcast on the 6-meter band. The frequency of this electromagnetic radiation is MHz. [speed of light

Volgvan

Answer:

50 MHz

Explanation:

The relation between frequency and wavelength is shown below as:

$c=frequency\times Wavelength$

c is the speed of light having value $3\times 10^8\ m/s$

Given, Wavelength = 6 m

Thus, Frequency is:

$Frequency=\frac{c}{Wavelength}$

$Frequency=\frac{3\times 10^8}{6}\ Hz$

$Frequency=50\times 10^{6}\ Hz$

Also,

Also, 1 Hz = $10^{-6}$ MHz

So,<u> Frequency = 50 MHz.</u>

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3 years ago

How many grams of H 2O are produced from 28.8 g of O 2? (Molar Mass of H 2O = 18.02 g) (Molar Mass of O 2=32.00 g) 4 NH 3 (g) +

krek1111 [17]

Answer: 13.9 g of $H_2O$ will be produced from the given mass of oxygen

Explanation:

To calculate the moles :

$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$

$\text{Moles of} O_2=\frac{28.8g}{32.00g/mol}=0.900moles$

The balanced chemical reaction is:

$4NIO_2(g)+7O_2(g)\rightarrow 4NO_2(g)+6H_2O(g)$

According to stoichiometry :

7 moles of $O_2$ produce = 6 moles of $H_2O$

Thus 0.900 moles of $O_2$ will produce = $\frac{6}{7}\times 0.900=0.771moles$ of $H_2O$

Mass of $H_2O=moles\times {\text {Molar mass}}=0.771moles\times 18.02g/mol=13.9g$

Thus 13.9 g of $H_2O$ will be produced from the given mass of oxygen

5 0

3 years ago

What is the chemical name of the compound KCN?

Monica [59]

Answer:Potassium cyanide

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3 years ago

He rate constant of a reaction is 4.55 × 10−5 l/mol·s at 195°c and 8.75 × 10−3 l/mol·s at 258°c. what is the activation energy o

Xelga [282]

Answer : The activation energy of the reaction is, $17.285\times 10^4kJ/mole$

Solution :

The relation between the rate constant the activation energy is,

$\log \frac{K_2}{K_1}=\frac{Ea}{2.303\times R}\times [\frac{1}{T_1}-\frac{1}{T_2}]$

where,

$K_1$ = initial rate constant = $4.55\times 10^{-5}L/mole\text{ s}$

$K_2$ = final rate constant = $8.75\times 10^{-3}L/mole\text{ s}$

$T_1$ = initial temperature = $195^oC=273+195=468K$

$T_2$ = final temperature = $258^oC=273+258=531K$

R = gas constant = 8.314 kJ/moleK

Ea = activation energy

Now put all the given values in the above formula, we get the activation energy.

$\log \frac{8.75\times 10^{-3}L/mole\text{ s}}{4.55\times 10^{-5}L/mole\text{ s}}=\frac{Ea}{2.303\times (8.314kJ/moleK)}\times [\frac{1}{468K}-\frac{1}{531K}]$

$Ea=17.285\times 10^4kJ/mole$

Therefore, the activation energy of the reaction is, $17.285\times 10^4kJ/mole$

8 0

3 years ago

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