Hi :) take some points for the road
2 answers:
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Hello user, you did not add a picture of an attachment to enable me help you solve this problem. Please check the attachment I added i believe it is the question that needs to be solved.
Explanation:
1. In the first column
<u>INCREASE CONCENTRATION</u>: these are the items that needs to be placed in this bin
a. Add drink mix solid to a diluted mixture of drink mix in pure water
b. Add drink mix solution to a diluted mixture of drink mix in pure water
c. Add drink mix solid to pure drink mix solution
d Evaporate water from a diluted mixture of drink mix in pure water
e Evaporate water from pure drink mix solution
2. The items below are what should be placed in this bin,<u>DECREASE CONCENTRATION:</u>
a. Add water to a diluted mixture of drink mix in pure water
b. Add water to pure drink mix solution
3. These items here should be placed here. <u>DOES NOT AFFECT CONCENTRATION:</u>
a. Add pure drink mix solution to pure drink mix solution
b. Drain the pure drink mix solution
c. Drain the diluted mixture
Answer:
The ideal gas equation
Explanation:
The ideal gas equation is derived from the combination of three gas laws:
- Boyle's law
- Charles's law
- Avogadro's law.
The ideal gas law is expressed mathematically as: PV=nRT where:
P is pressure
V is volume
n is the number of moles
R is the ideal gas law
T is temperature.
To obtain the combined gas law, we assume that n=1 and this gives:
= R
Therefore:
=
Answer: -
12.41 g
Explanation: -
Mass of CO₂ = 42 g
Molar mass of CO₂ = 12 x 1 + 16 x 2 = 44 g / mol
Number of moles of CO₂ =
= 0.9545 mol
The balanced chemical equation for this process is
2C₆H₆ + 15O₂ → 12CO₂ + 6H₂O
From the balanced chemical equation we see
12 mol of CO₂ is produced from 2 mol of C₆H₆
0.9545 mol of CO₂ is produced from
= 0.159 mol of C₆H₆
Molar mass of C₆H₆ = 12 x 6 + 1 x 6 =78 g /mol
Mass of C₆H₆ =Molar mass x Number of moles
= 78 g / mol x 0.159 mol
= 12.41 g