2 Points<br><br> Which of these is a benefit of using cotton grocery bags?

15. What is true about concentration of a solution? *

Naya [18.7K]

<h3>Answer:</h3>

A saturated solution is a chemical solution containing the maximum concentration of a solute dissolved in the solvent.

<h3>Explanation:</h3>

A solution is made by dissolving a solute in a solvent.
For example dissolving a salt in a solvent such as water results to a solution.
Solution may either be saturated or unsaturated.
Unsaturated solution is a solution that can dissolve more solute upon addition because it has not reached saturation.
A saturated solution on the other hand is a solution that has maximum solute and the concentration of solute is maximum and thus the solvent can not dissolve any more solute.
Therefore, a saturated solutions contain maximum concentration of a solute dissolved in the solute.

8 0

3 years ago

Katyanochek1 [597]

Answer:

The answer to your question is V2 = 4.97 l

Explanation:

Data

Volume 1 = V1 = 4.40 L Volume 2 =

Temperature 1 = T1 = 19°C Temperature 2 = T2 = 37°C

Pressure 1 = P1 = 783 mmHg Pressure 2 = 735 mmHg

Process

1.- Convert temperature to °K

T1 = 19 + 273 = 292°K

T2 = 37 + 273 = 310°K

2.- Use the combined gas law to solve this problem

P1V1/T1 = P2V2/T2

-Solve for V2

V2 = P1V1T2 / T1P2

-Substitution

V2 = (783 x 4.40 x 310) / (292 x 735)

-Simplification

V2 = 1068012 / 214620

-Result

V2 = 4.97 l

6 0

3 years ago

The reaction of NO2 with ozone produces NO3 in a second-order reaction overall.

Brilliant_brown [7]

Answer : The rate of reaction is,

$Rate=4.77\times 10^{-19}M/s$

The appearance of $NO_3$ is, $4.77\times 10^{-19}M/s$

Explanation :

The general rate of reaction is,

$aA+bB\rightarrow cC+dD$

Rate of reaction : It is defined as the change in the concentration of any one of the reactants or products per unit time.

The expression for rate of reaction will be :

$\text{Rate of disappearance of A}=-\frac{1}{a}\frac{d[A]}{dt}$

$\text{Rate of disappearance of B}=-\frac{1}{b}\frac{d[B]}{dt}$

$\text{Rate of formation of C}=+\frac{1}{c}\frac{d[C]}{dt}$

$\text{Rate of formation of D}=+\frac{1}{d}\frac{d[D]}{dt}$

$Rate=-\frac{1}{a}\frac{d[A]}{dt}=-\frac{1}{b}\frac{d[B]}{dt}=+\frac{1}{c}\frac{d[C]}{dt}=+\frac{1}{d}\frac{d[D]}{dt}$

From this we conclude that,

In the rate of reaction, A and B are the reactants and C and D are the products.

a, b, c and d are the stoichiometric coefficient of A, B, C and D respectively.

The negative sign along with the reactant terms is used simply to show that the concentration of the reactant is decreasing and positive sign along with the product terms is used simply to show that the concentration of the product is increasing.

The given rate of reaction is,

$NO_2(g)+O_3(g)\rightarrow NO_3(g)+O_2(g)$