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Andru [333]
3 years ago
14

How many milliliters of pure liquid methanol (ch3oh, mw = 32.04 g/mol) are needed to prepare 500.0 ml of an aqueous solution of

12.0 g/l methanol? the density of pure liquid methanol is 0.791 g/ml?
Chemistry
1 answer:
Nookie1986 [14]3 years ago
4 0

Answer:- 7.59 mL.

Solution:- We want to make 500.0 mL of an aqueous solution of methanol whose density is 12.0\frac{g}{L}. This has to be made from a given pure liquid methanol with density 0.791\frac{g}{mL} . It asks to calculate the volume of pure liquid methanol.

We know that, mass = volume*density

Let's calculate the mass of aqueous solution from it's given volume and density. need to convert volume unit from mL to L as the density is given in grams per liter:

mass of aqueous methanol solution = 500.0mL(\frac{1L}{1000mL})(\frac{12.0g}{L})

= 6 g

From above calculations, we need to use 6 g of pure liquid methanol. It's density is known, so we could calculate it's volume as:

volume=\frac{mass}{density}

Let's plug in the values in it:

volume=6g(\frac{1mL}{0.791g})

= 7.59 mL

Hence, we need to take 7.59 mL of pure liquid methanol.

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Determine the value of the equilibrium constant, Kgoal, for the reaction C(s)+12O2(g)+H2(g)⇌12CH3OH(g)+12CO(g), Kgoal=? by makin
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Answer:

1.71x10²⁷

Explanation:

If we sum 1/2 of (3) + 1/2 of (1):

1/2 (3.) C(s) + 1/2O₂(g) ⇌ CO(g), K₃ = √2.10×10⁴⁷  = 4.58x10²³

1/2 (1)   1/2CO₂(g) + 3/2H₂(g) ⇌ 1/2CH₃OH(g) + 1/2H₂O(g), K₁ = √1.40×10² = 11.8

C(s) + 1/2O₂(g) +<u> 1/2CO₂(g) </u>+<u> 3/2H₂(g</u>) ⇌ 1/2CH₃OH(g) + <u>1/2H₂O(g)</u> + <u>CO(g)</u>

K' = 4.58x10²³ * 11.8 = 5.42x10²⁴

+1/2 (2):

<u>1/2 CO(g)</u> +<u> 1/2H₂O(g)</u> ⇌<u> 1/2CO₂(g)</u> + <u>1/2H₂</u> (g), K = √1.00×10⁵ = 316.2

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K'' = 5.42x10²⁴* 316.2 =

<h3>1.71x10²⁷</h3>

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3 years ago
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