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2 years ago

What is the balanced form fir Na(s) + ao2(g) = Na2O(s)

Chemistry

1 answer:

Dima020 [189]2 years ago

6 0

Answer:

Balanced Chemical equation:

4Na + O₂ → 2Na₂O

Explanation:

Chemical equation:

Na + O₂ → Na₂O

Balanced Chemical equation:

4Na + O₂ → 2Na₂O

Four mole of sodium combine with one mole of oxygen and form two mole of sodium oxide.

Coefficient with reactant and products:

Na 4

O₂ 1

Na₂O 2

Oxygen is present in group sixteen and have six valance electrons. while sodium is alkali metal and present in group one and have one valance electron.

Oxygen needs two electron to complete the octet while sodium need to lose the one electron to get the complete octet.

When oxygen is combine with sodium it gain its two valance electrons from two sodium atom and form anion while sodium loses its valance electron to wards oxygen and form cation. The bond form between them is ionic because one is metal and other is non metal and electrons are completely transfer from two sodium atom to one oxygen atom.

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A 3.301 mass % aqueous solution of potassium hydroxide has a density of 1.05 g/mL. Calculate the molality of the solution. Give

8_murik_8 [283]

Answer: The molality of potassium hydroxide solution is 0.608 m

Explanation:

We are given:

3.301 mass % of potassium hydroxide solution.

This means that 3.301 grams of potassium hydroxide is present in 100 grams of solution

Mass of solvent = Mass of solution - Mass of solute (KOH)

Mass of solvent = (100 - 3.301) g = 96.699 g

To calculate the molality of solution, we use the equation:

$\text{Molality}=\frac{m_{solute}\times 1000}{M_{solute}\times W_{solvent}\text{ (in grams})}$

Where,

$m_{solute}$ = Given mass of solute (KOH) = 3.301 g

$M_{solute}$ = Molar mass of solute (KOH) = 56.1 g/mol

$W_{solvent}$ = Mass of solvent = 96.699 g

Putting values in above equation, we get:

$\text{Molality of KOH}=\frac{3.301\times 1000}{56.1\times 96.699}\\\\\text{Molality of KOH}=0.608m$

Hence, the molality of potassium hydroxide solution is 0.608 m

4 0

2 years ago

A gas exerts a pressure of 1.8 atm at a temperature of 60 degrees celsius. What is the new temperature when the pressure of the

Kamila [148]

The answer for the following problem is mentioned below.

Therefore the final temperature of the gas is 740 K

Explanation:

Given:

Initial pressure of the gas ( $P_{1}$ ) = 1.8 atm

Final pressure of the gas ( $P_{2}$ ) = 4 atm

Initial temperature of the gas ( $T_{1}$ ) = 60°C = 60 + 273 = 333 K

To solve:

Final temperature of the gas ( $T_{2}$ )

We know;

From the ideal gas equation;

we know;

P × V = n × R × T

So;

we can tell from the above equation;

P ∝ T

(i.e.)

$\frac{P}{T}$ = constant

$\frac{P_{1} }{P_{2} }$ = $\frac{T_{1} }{T_{2} }$

Where;

$P_{1}$ = initial pressure of a gas

$P_{2}$ = final pressure of a gas

$T_{1}$ = initial temperature of a gas

$T_{2}$ = final temperature of a gas

$\frac{1.8}{4}$ = $\frac{333}{T_{2} }$

$T_{2}$ = $\frac{333*4}{1.8}$

$T_{2}$ = 740 K

Therefore the final temperature of the gas is 740 K

8 0

3 years ago

Help me please!!! HELP ME

Neporo4naja [7]

Answer:

Its a

Explanation:

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2 years ago

What is the balanced form fir Na(s) + ao2(g) = Na2O(s)​

What is the balanced form fir Na(s) + ao2(g) = Na2O(s)