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KIM [24]
3 years ago
5

Muddy water is what type of solution

Chemistry
1 answer:
Zielflug [23.3K]3 years ago
4 0
It is an heterogeneous solution.
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Please someone help me to solve this problem​
Zinaida [17]

Answer:

(a) The final pressure of the sample becomes one-fourth of the original pressure.

(b) The pressure of the sample remains unchanged.

(c) The final pressure of the sample becomes four times of the original pressure.

Explanation:

(a)

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

The volume of sample doubled and kelvin temperature halved.

V_{2}=2V_{1}

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

P_{2}=\frac{P_{1}\times V_{1}\times \frac{1}{2}T_{1}}{T_{1}\times2V_{1}}=\frac{P_{1}}{4}

Therefore, the final pressure of the sample becomes one-fourth of the original pressure.

(b)

Volume and temperature of sample doubled.

V_{2}=2V_{1}

T_{2}=2T_{1}

P_{2}=\frac{P_{1}\times V_{1}\times 2T_{1}}{T_{1}\times2V_{1}}={P_{1}}

Therefore, the pressure of the sample unchanged.

(c)

Volume of sample halved and temperature double.

V_{2}=\frac{1}{2}V_{1}

T_{2}=2T_{1}

P_{2}=\frac{P_{1}\times V_{1}\times 2T_{1}}{T_{1}\times \frac{1}{2}V_{1}}={4P_{1}}

Therefore, the pressure of the sample becomes four times of the original pressure.

6 0
3 years ago
The reaction of an acid and a base will always produce what kind of salt?
Musya8 [376]

Explanation:

E maybe i am not sure or C

4 0
3 years ago
Why did one liter of nitrogen prepared by lord rayleigh appear to have a greater mass than the other liter prepared by a differe
Snowcat [4.5K]
There were two methods that Lord Rayleigh used in his experiment. First, nitrogen was obtained from the atmosphere by passing air over hot copper. Second, air was bubbled through an ammonia mixture, then passed over hot copper. The second method would have a greater mass of nitrogen than the first, <em>because the nitrogen from the atmosphere was contaminated by the nitrogen from the ammonia mixture.</em>
8 0
3 years ago
. A Chemist wants to make 20moles of Hydrogen gas by combining Calcium with water. Balanced Chemical Reaction: 2 Ca(s) + 2H20 -&
german

Answer:

92 moles in 1 gram

hope this helps

3 0
2 years ago
You start with an equimolar mixture of the gases SO₂ and O₂ in a container. The SO₂ and O₂ react to completion to form SO₃. If t
LuckyWell [14K]

The density of the product gas mixture is 5.39 g/L

Explanation:

<u>Given:</u>

Temperature after the reaction = 25^0C

Pressure in the container = 1.65 atm

The ideal gas equation PV = nRT

<u>To find:</u> Density of the product gas mixture

<u>Step 1:</u>

Molarity (M) = P/(RT)

\[M=\frac{P}{R T}\]$M=\frac{1.65 \mathrm{atm}}{\left(0.08206 \frac{L \cdot a t m}{m o l . K}\right)(298.15 K)}$

M = 0.0674 mol/L

<u>Step 2: </u>

The product of the given reaction is SO_3. Its molar mass is

1S x 32.066 g/mol = 32.066 g/mol

3O x 16 g/mol = 48 g/mol

Adding both we get 80.066 g/mol

Therefore the density of the product gas mixture is 0.0674 \frac{{mol}}{L} \times \frac{80.066 g}{1 \mathrm{mol}}

= 5.39 g/L

8 0
3 years ago
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