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Kazeer [188]
3 years ago
11

If 35.8 grams of LiCl are dissolved in 184 grams of water, what is the concentration of the solution in percent by mass?

Chemistry
2 answers:
aleksandrvk [35]3 years ago
4 0

I recieved 16.3% as my answer.

True [87]3 years ago
3 0
35.8/184=.194565, or 19.4565%
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3 years ago
Please help no links
jarptica [38.1K]

Answer:

23 L

Explanation:

We'll begin by converting celsius temperature to Kelvin temperature. This can be obtained as follow:

T(K) = T(°C) + 273

Initial temperature (T₁) = 100 °C

Initial temperature (T₁) = 100 °C + 273

Initial temperature (T₁) = 373 K

Final temperature (T₂) = 50.5 °C

Final temperature (T₂) = 50.5 °C + 273

Final temperature (T₂) = 323.5 K

Finally, we shall determine the initial volume of gas. This can be obtained as follow:

Initial temperature (T₁) = 373 K

Final temperature (T₂) = 323.5 K

Final volume (V₂) = 20 L

Initial volume (V₁) =?

V₁/T₁ = V₂/T₂

V₁ / 373 = 20 / 323.5

Cross multiply

V₁ × 323.5 = 373 × 20

V₁ × 323.5 = 7460

Divide both side by 323.5

V₁ = 7460 / 323.5

V₁ = 23 L

Thus, the original volume of the gas is 23 L

7 0
2 years ago
How many moles of water are<br> in 1.23x1018 water molecules?
sesenic [268]

Answer:

0.20 times 10(-5)

Explanation:

5 0
3 years ago
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Juliette [100K]

Answer:

C

Explanation:

O2 is a gas and gas has spread out molecules compared to the other states of matter. As such, liquid and solids have stronger intermolecular forces. Since dioxygen is the only gas in the possible answers, O2 has the weakest intermolecular force.

3 0
3 years ago
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An aerosol can contains 350.mL of gas at a pressure of 5.00 atm. What would be the volume of the gas at 2.00atm?
Margaret [11]

Answer:

<h2>875 mL</h2>

Explanation:

The new volume can be found by using the formula for Boyle's law which is

P_1V_1 = P_2V_2

Since we are finding the new volume

V_2 =  \frac{P_1V_1}{P_2}  \\

From the question we have

V_2 =  \frac{350 \times 5}{2}  =  \frac{1750}{2}  \\

We have the final answer as

<h3>875 mL</h3>

Hope this helps you

8 0
3 years ago
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