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DanielleElmas [232]
2 years ago
9

What is the volume of 0.20 moles of helium at STP?

Chemistry
1 answer:
SOVA2 [1]2 years ago
7 0

Answer:

Option (C) 4.5 liters

Explanation:

1mole of a gas occupy 22.4L at stp.

This implies that 1mole of He also occupy 22.4L at stp.

From the question given, we were asked to find the volume occupied by 0.20 mole of He at STP. This can be achieved by doing the following:

1mole of He occupied 22.4L.

Therefore, 0.2mol of He will occupy = 0.2 x 22.4L = 4.48 = 4.5L

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NEED ASAP!
Harlamova29_29 [7]

Answer:

discoveries that can change little aspects of our daily lives or finding cures for diseases that have hounded humanity, scientists have been hard at work trying to push us toward a brighter future.

Explanation:

thats what i got from my research :D

7 0
2 years ago
Some people believe that the Moon’s phases are caused by Earth’s shadows on the Moon. Is this true? Use your model to explain.
Kisachek [45]

<u>Answer:</u>   False

<em>Some people believe that the Moon’s phases are caused by Earth’s shadows on the Moon is false.</em>

<u>Explanation:</u>

<em>Some people believe that the Moon’s phases are caused by Earth’s shadows on the Moon is their misconception. </em>

The phases depend on its place relative with sun and earth.The phases of moon are new moon,waxing crescent, first quarter, waxing gibbon, full moon, wanning gibbon,last quarter, wanning crescent,new moon.

<em>For example, </em>

When<em> moon, earth, and sun</em> are exactly in the same line and moon lies in between earth and sun, the sun illuminates the back part of the moon which is not visible from earth. <em>This forms new moon</em>.

<em>So only relative positions matter in the phases of moon. </em>

5 0
2 years ago
When silver nitrate is added to the Fe/SCN equilibrium, why is the colorless intense and a precipitate forms?
Reptile [31]

Answer:

Here's what I get  

Explanation:

You have an equilibrium reaction between Fe³⁺/ SCN⁻ and FeSCN²⁺.

\underbrace{\hbox{Fe$^{3+}$}}_{\text{pale yellow-green}} +\underbrace{\hbox{SCN$^{-}$}}_{\text{colourless}} \, \rightleftharpoons \, \underbrace{\hbox{Fe(SCN)$^{2+}$}}_{\text{deep blood red}} \\

When you add AgNO₃, the Ag⁺ reacts with the SCN⁻. It forms a colourless precipitate of Ag(SCN).

Ag⁺(aq) + SCN⁻(aq) ⟶ AcSCN(s)

According to Le Châtelier's Principle, when we apply a stress to a system at equilibrium, the system will respond in a way that tends to relieve the stress.

If you add Ag⁺ to the equilibrium solution, it removes the SCN⁻ [as an Ag(SCN) precipitate].

The system responds by trying to replace the missing SCN⁻:

The Fe(SCN)²⁺ dissociates to form SCN⁻, so the position of equilibrium shifts to the left,

You now have more Fe³⁺ and SCN⁻ and less of the highly coloured Fe(SCN)²⁺ at the new equilibrium.

The deep red colour becomes less intense.

 

3 0
3 years ago
A water treatment tablet contains 20.0 mg of tetraglycine hydroperiodide, 40.0% of which is available as soluble iodine. If two
Galina-37 [17]

Answer:

16\ \text{ppm}

Explanation:

Mass of one tablet = 20 mg

Mass of two tablets = 2\times 20=40\ \text{mg}

Percent that is soluble in water = 40%

Mass of tablet that is soluble in water = 0.4\times 40=16\ \text{mg}

So, mass of solute is 16\ \text{mg}

Density of water = 1 kg/L

Volume of water = 1 L

So, mass of 1 L of water is 1\times 1=1\ \text{kg}=1000\ \text{g}

PPM is given by

\dfrac{\text{Mass of solute}}{\text{Mass of solvent}}\times 10^6=\dfrac{16\times 10^{-3}}{1000}\times 10^6\\ =16\ \text{ppm}

Hence, the concentration of iodine in the treated water 16\ \text{ppm}.

8 0
3 years ago
Sodium azide, NaN3, the explosive compound found in automobile air bags, decomposes according to the following equation: 2NaN3(s
shutvik [7]

Answer:

1.9 × 10² g NaN₃

1.5 g/L

Explanation:

Step 1: Write the balanced decomposition equation

2 NaN₃(s) ⇒ 2 Na(s) + 3 N₂(g)

Step 2: Calculate the moles of N₂ formed

N₂ occupies a 80.0 L bag at 1.3 atm and 27 °C (300 K). We will calculate the moles of N₂ using the ideal gas equation.

P × V = n × R × T

n = P × V / R × T

n = 1.3 atm × 80.0 L / (0.0821 atm.L/mol.K) × 300 K = 4.2 mol

We can also calculate the mass of nitrogen using the molar mass (M) 28.01 g/mol.

4.2 mol × 28.01 g/mol = 1.2 × 10² g

Step 3: Calculate the mass of NaN₃ needed to form 1.2 × 10² g of N₂

The mass ratio of NaN₃ to N₂ is 130.02:84.03.

1.2 × 10² g N₂ × 130.02 g NaN₃/84.03 g N₂ = 1.9 × 10² g NaN₃

Step 4: Calculate the density of N₂

We will use the following expression.

ρ = P × M / R × T

ρ = 1.3 atm × 28.01 g/mol / (0.0821 atm.L/mol.K) × 300 K = 1.5 g/L

5 0
2 years ago
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