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3 years ago

How many ammonium ions, nh4 , are there in 5.0 mol (nh4)2s?

Chemistry

2 answers:

aleksandr82 [10.1K]3 years ago

5 0

Answer: The number of ammonium ions in given moles of ammonium sulfide are $6.022\times 10^{24}$

Explanation:

We are given:

A chemical compound having chemical formula of $(NH_4)_2S$

In 1 mole of ammonium sulfide, 2 moles of ammonium ions and 1 mole of sulfide ions are present.

According to mole concept:

1 mole of compound contains $6.022\times 10^{23}$ number of atoms

So, 5 moles of ammonium sulfide molecule will contain = $5\times 2\times 6.022\times 10^{23}=6.022\times 10^{24}$ number of ammonium ions.

Hence, the number of ammonium ions in given moles of ammonium sulfide are $6.022\times 10^{24}$

olchik [2.2K]3 years ago

3 0

There are two such ions in every molecule
1 mol contains 6.02 * 10^23 things.
1 mol of (NH4)2S contains 2*6.02 * 10^23 ions (of NH4+ in this case.) = 1.204 * 10^24 ions HN4+

5 mol of (NH4)2S contains 5 * 1.204*10^24 =
6.02 * 10^24 mols NH4+ions <<<<====Answer

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A circuit breaker must be replaced after too much current flowing through it causing it to melt.

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2 years ago

Write a balanced equation for the reaction between ammonia and sulfuric acid?

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2 years ago

The electron configurations of two unknown elements x and y are shown. X: 1s2 2s2 2p6 Y: 1s2 2s2 2p6 3s2 3p6 Which statement is

SVETLANKA909090 [29]

Answer:

B) They will react because X and Y can share two pairs of electrons to become stable

Explanation:

The electron configurations of two elements x and y are given :

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Y: 1s2 2s2 2p6 3s2 3p6

The statement that is true for both the elements is that, they both will react as they both can share two pairs of electrons to become stable.

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2 years ago

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

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zavuch27 [327]

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3 years ago