A flat metal surface in an electric cell is its ________

An oxide of nitrogen contains 30.45 mass % N.

N76 [4]

An oxide of nitrogen contains 30.45 mass % N, if the molar mass is 90± 5 g/mol the molecular formula is N₂O₄.

<h3>What is molar mass?</h3>

The molar mass of a chemical compound is determined by dividing its mass by the quantity of that compound, expressed as the number of moles in the sample, measured in moles. A substance's molar mass is one of its properties. The compound's molar mass is an average over numerous samples, which frequently have different masses because of isotopes.

<h3>How to find the molecular formula?</h3>

The whole-number multiple is defined as follows.

Whole-number multiple = $\frac{molar mass (g/mol)}{empirical formula mass (g/mol)}$

The empirical formula mass is shown below.

Mw of empirical formula = Mw of N+ 2 x (Mw of O)

= 14.01 g/mol + 2 x (16.00 g/mol)

= 46.01 g/mol

With the given molar mass or the molecular formula mass, we can get the whole-number multiple for the compound.

Whole-number multiple = $\frac{90 g/mol }{46.01 g/mol}$ ≈ 2

Multiplying the subscripts of NO2 by 2, the molecular formula is N(1x2)O(2x2)= N2O4.

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5 0

2 years ago

How does molecular shape affect polarity?

Andrej [43]

Answer:

Letter D

Explanation:

6 0

2 years ago

Read 2 more answers

Ome fire extinguishers contain liquid carbon dioxide Suggest how carbon dioxide

melisa1 [442]

Answer:

The CO2 Extinguisher Cannisters contain carbon dioxide in liquid form, and when the extinguisher is let off the liquid is released into the air neutralising the oxygen that the fire is feeding on, disabling the fires ability to spread.

8 0

3 years ago

In a titration of 47.41 mL of 0.3764 M ammonia with 0.3838 M aqueous nitric acid, what is the pH of the solution when 47.41 mL +

Volgvan

<u>Answer:</u> The pH of the solution is 1.136

<u>Explanation:</u>

To calculate the moles from molarity, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}$

<u>For ammonia:</u>

Molarity of ammonia = 0.3764 M

Volume of ammonia = 47.41 mL = 0.04741 L (Conversion factor: 1 L = 1000 mL)

Putting values in above equation, we get:

$0.3764mol/L=\frac{\text{Moles of ammonia}}{0.04741L}\\\\\text{Moles of ammonia}=0.01784mol$

<u>For nitric acid:</u>

Molarity of nitric acid = 0.3838 M

Volume of ammonia = (47.41 + 10.00) mL = 57.41 mL= 0.05741 L

Putting values in above equation, we get:

$0.3838mol/L=\frac{\text{Moles of nitric acid}}{0.05741L}\\\\\text{Moles of nitric acid}=0.02203mol$

After the completion of reaction, amount of nitric acid remained = 0.022 - 0.0178 = 0.0042 mol

For the reaction of ammonia with nitric acid, the equation follows:

$NH_3+HNO_3\rightarrow NH_4NO_3$

At $t=0$ 0.0178 0.022

Completion 0 0.0042 0.0178

As, the solution of the reaction is made from strong acid which is nitric acid and the conjugate acid of weak base which is ammonia. So, the pH of the reaction will be based totally on the concentration of nitric acid.

To calculate the pH of the reaction, we use the equation:

$pH=-\log[H^+]$