Answer:
13.687 grams of salt should be added
The total grams of 8.6% of brine solution produced is 852.687g
Explanation:
Solution mass= 962g
Salt= 6.2%
Water = 93.8%
962 gram of water is made up of:
902.356g ( due to vaporization which reduces mass)
= 902.356 - 123
= 779. 356g of water
59.644g of salt.
If we add x gram of salt for making brine solution up to 8.6%
=(59. 644g + x)g.of salt
% salt = Mass of Salt / Total mass of solution
= 0.086= 59.644 + x / 779.356 + 59.644 + x
= 59.644 + x / 839 + x
x= 13.687 g of salt
Grams of 8.6% brine solution will be:
Gram of water + total gram of salt added to form 8.6% brine solution.
= 779.356g +59.644g + 13.687g
= 852.687g
The total grams of 8.6% of brine solution produced is 852.687g
<span>If the water faucet is opened, then the amount of water flowing will increase. </span>
Answer: The conversion to malate
Explanation:
Pyruvate is the process which produced in glycoysis which has multiple fates and it can give rises to acetyl co-enzyme and undergo the aerobic oxidation in the critic acid cycle. It can be used to produces glucose but it never produced the malate. In prokaryotes it can be processes in the anaerobic respiration to produced the ethanol, as end product.
Answer:
A) 31.22
Explanation:
The reaction of sulfuric acid with NaOH is:
H₂SO₄ + 2 NaOH → Na₂SO₄ + 2H₂O
To solve this problem we need to determine the moles of acid that will react, and, using the chemical equation we can determine the moles of NaOH and the volume that a 0.2389M NaOH solution would require to neutralize it.
<em>Moles H₂SO₄ (Molar mass: 98.08g/mol):</em>
0.9368g * 39.04% = 0.3657g H₂SO₄ * (1mol / 98.08g) =
3.7289x10⁻³moles H₂SO₄
And moles of NaOH that you require to neutralize the acid are:
3.7289x10⁻³moles H₂SO₄ * (2 moles NaOH / 1 mole H₂SO₄) =
7.4578x10⁻³ moles NaOH
Using a 0.2389M NaOH solution:
7.4578x10⁻³ moles NaOH * (1L / 0.2389mol) = 0.03122L = 31.22mL
Right answer is:
<h3>A) 31.22
</h3>
Answer : The partial pressure of the hydrogen is, 705.9 mmHg
Explanation :
According to the Dalton's law of partial pressure,
where,
= total pressure of the gas = 729.7 mmHg
= partial pressure of the hydrogen gas = ?
= partial pressure of the water = 23.8 mmHg (standard value)
Now put all the given values in the above expression, we get:
Therefore, the partial pressure of the hydrogen is, 705.9 mmHg
