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2 years ago

In this equilibrium, hydroxide ion acts as a A) Lewis base B) Bronsted base C) both A & B D) neither A or B

Chemistry

1 answer:

Nata [24]2 years ago

5 0

Answer:

(b) Bronsted base

Explanation:

The hydroxide ion is formed when $H_2O$ losses $H^+$ ion

We know hat the compound which losses $H^+$ is known as the bronsted acid and the ion which is formed after losing $H^+$ is known as bronsted base

As the hydroxide ion is formed after losing the hydrogen ion from $H_2O$ so it is a bronsted base.

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Veseljchak [2.6K]

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A gas used to extinguish fires is composed of 75 % CO2 and 25 % N2. It is stored in a 5 m3 tank at 300 kPa and 25 °C. What is th

tatyana61 [14]

Answer : The partial pressure of the $CO_2$ in the tank in psia is, 32.6 psia.

Explanation :

As we are given 75 % $CO_2$ and 25 % $N_2$ in terms of volume.

First we have to calculate the moles of $CO_2$ and $N_2$ .

$\text{Moles of }CO_2=\frac{\text{Volume of }CO_2}{\text{Volume at STP}}=\frac{75}{22.4}=3.35mole$

$\text{Moles of }N_2=\frac{\text{Volume of }N_2}{\text{Volume at STP}}=\frac{25}{22.4}=1.12mole$

Now we have to calculate the mole fraction of $CO_2$ .

$\text{Mole fraction of }CO_2=\frac{\text{Moles of }CO_2}{\text{Moles of }CO_2+\text{Moles of }N_2}$

$\text{Mole fraction of }CO_2=\frac{3.35}{3.35+1.12}=0.75$

Now we have to calculate the partial pressure of the $CO_2$ gas.

$\text{Partial pressure of }CO_2=\text{Mole fraction of }CO_2\times \text{Total pressure of gas}$

$\text{Partial pressure of }CO_2=0.75mole\times 300Kpa=225Kpa=225Kpa\times \frac{0.145\text{ psia}}{1Kpa}=32.625\text{ psia}$

conversion used : (1 Kpa = 0.145 psia)

Therefore, the partial pressure of the $CO_2$ in the tank in psia is, 32.6 psia.

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2 years ago

In H2 (g) + I2 (g) = 2HI (g), the initial reactions H2 and I2 are each equal to 1 mol / L.

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Answer:

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2 years ago

1 Define Soft water and Hard water.

madreJ [45]

Answer

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Explanation:

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2 years ago