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Georgia [21]
3 years ago
15

What happened to solid materials when mixed with the liquid materials?​

Chemistry
2 answers:
KonstantinChe [14]3 years ago
5 0

Answer:

the solid materials will disappear after mixing with a liquid material

plsss mark me as brainliest answer plsssssssss

agasfer [191]3 years ago
5 0

Answer: go fk your dad you fkin whor

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Two containers, one with a volume of 3.0 L and the other with a volume of 2.0 L contain, respectively, argon gas at 1.1 atm and
aalyn [17]

Answer:

a. p_T=0.93atm.

b.

p_{Ar}=0.66atm\\\\p_{He}=0.3atm

c.

x_{Ar}=0.6875\\\\x_{He}=0.3125

Explanation:

Hello,

In this case, considering that the valve is opened, we can use the Boyle's law in order to compute the final pressure of argon by considering its initial pressure and volume and a final volume of 5.0 L:

p_{Ar}=\frac{1.1atm*3.0L}{5.0L}=0.66atm

And the final pressure of helium:

p_{He}=\frac{0.75atm*2.0L}{5.0L}=0.3atm

Which actually are the partial pressure of both of them, it means that the total pressure is:

Finally, the mole fraction of each gas is computed by considering the Dalton's law:

x_i=\frac{p_i}{p_T}

x_{Ar}=\frac{0.66atm}{0.93atm} =0.6875\\\\x_{He}=\frac{0.3atm}{0.93atm} =0.3125

Best regards.

6 0
3 years ago
What is the atomic number and name of an element that has 15 protons in its nucleus?
just olya [345]

Answer:

phosphorus.

Explanation:

The atomic number of phosphorus is 15 so the protons will be 15.

4 0
3 years ago
Read 2 more answers
PLEASE HELP!!
grandymaker [24]

Answer:

1. 136 °C.

2. 0.21 atm.

Explanation:

1. Determination of the new temperature in °C.

Initial volume (V1) = 1.35L

Final volume (V2) = 1.95L

Initial temperature (T1) = 283 K

Final temperature (T2) =...?

Using the Charles' law equation, the new temperature of the gas can be obtained as follow:

V1 /T1 = V2 /T2

1.35/283 = 1.95/T2

Cross multiply

1.35 × T2 = 283 × 1.95

1.35 × T2 = 551.85

Divide both side by 1.35

T2 = 551.85/1.35

T2 = 408.8 ≈ 409 K

Finally, we shall convert 409 K to °C. This can be obtained as follow:

T (°C) = T(K) – 273

T(K) = 409 K

T (°C) = 409 – 273

T (°C) = 136 °C

Therefore, the new temperature of the gas is 136 °C.

2. Determination of the new pressure.

Initial pressure (P1) = 1.34 atm

Initial volume (V1) = 267 mL

Final volume (V2) = 1.67 L

Final pressure (P2) =.?

Next, we shall convert 1.67 L to millilitres (mL). This can be obtained as follow:

1 L = 1000 mL

Therefore,

1.67 L = 1.67 L × 1000 mL / 1 L

1.67 L = 1670 mL

Therefore, 1.67 L is equivalent to 1670 mL.

Finally, we shall determine the new pressure of the gas as follow:

Initial pressure (P1) = 1.34 atm

Initial volume (V1) = 267 mL

Final volume (V2) = 1670 mL

Final pressure (P2) =.?

P1V1 = P2V2

1.34 × 267 = P2 × 1670

357.78 = P2 × 1670

Divide both side by 1670.

P2 = 357.78 / 1670

P2 = 0.21 atm.

Therefore, the new pressure of the gas is 0.21 atm.

3 0
3 years ago
PLEASE HELP QUICK!
Mila [183]

Answer:A

Explanation:

Your muscular system is at work

6 0
2 years ago
The chemical bonds in sugar
zhannawk [14.2K]

Sugar, on the other hand, is composed of carbon, oxygen, and hydrogen and has covalent bonds. A salt molecule is made up of one sodium atom and one chlorine atom.

8 0
3 years ago
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