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timama [110]
2 years ago
8

What change would increase the amount of solid solute able to be dissolved in liquid water?

Chemistry
1 answer:
exis [7]2 years ago
3 0
Bonjour,

increasing temperature.
for many solids dissolved in liquid water, the solubility increases with temperature.
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What is the mass of 0.60 moles of Al
KIM [24]

16 g. The mass of 0.60 mol Al is 16 g.

Molar mass of Al = 26.98 g/mol

Mass of Al = 0.60 mol Al x (26.98 g Al/1 mol Al) = 16 g Al

6 0
3 years ago
Read 2 more answers
RATE LAW QUESTION !
vivado [14]
In general, we have this rate law express.:

\mathrm{Rate} = k \cdot [A]^x [B]^y
we need to find x and y

ignore the given overall chemical reaction equation as we only preduct rate law from mechanism (not given to us).

then we go to compare two experiments in which only one concentration is changed

compare experiments 1 and 4 to find the effect of changing [B]
divide the larger [B] (experiment 4)  by the smaller [B] (experiment 1) and call it Δ[B]

Δ[B]= 0.3 / 0.1 = 3

now divide experiment 4 by experient 1 for the given reaction rates, calling it ΔRate:

ΔRate = 1.7 × 10⁻⁵ / 5.5 × 10⁻⁶ = 34/11 = 3.090909...

solve for y in the equation \Delta \mathrm{Rate} = \Delta [B]^y

3.09 = (3)^y \implies y \approx 1

To this point, \mathrm{Rate} = k \cdot [A]^x [B]^1

do the same to find x.
choose two experiments in which only the concentration of B is unchanged:

Dividing experiment 3 by experiment 2:
Δ[A] = 0.4 / 0.2 = 2
ΔRate = 8.8 × 10⁻⁵ / 2.2 × 10⁻⁵ = 4

solve for x for \Delta \mathrm{Rate} = \Delta [A]^x

4=  (2)^x \implies x = 2

the rate law is

Rate = k·[A]²[B]
6 0
2 years ago
2. Calculate the number-average molecular weight of a random poly (isobutylene-isoprene) copolymer in which the fraction of isob
Phoenix [80]

Answer : The number-average molecular weight is, 97500 g/mol

Explanation :

First we have to calculate the molecular weight of isobutylene and isoprene.

The molecular formula of isobutylene and isoprene is, C_4H_8 and C_5H_8

Molecular weight of C_4H_8 = 4(12 g//mol) + 8(1 g/mol) = 56 g/mol

Molecular weight of C_5H_8 = 5(12 g//mol) + 8(1 g/mol) = 68 g/mol

Now we have to calculate the average repeat molecular weight.

Average repeat molecular weight = 0.25\times (56g/mol)+(1-0.25)\times (68g/mol)

Average repeat molecular weight = 65 g/mol

Now we have to calculate the number-average molecular weight.

Number-average molecular weight = Average repeat molecular weight × Degree of polymerization

Number-average molecular weight = (65 g/mol) × (1500)

Number-average molecular weight = 97500 g/mol

Thus, the number-average molecular weight is, 97500 g/mol

5 0
3 years ago
The compound adrenaline contains 56.7 % c, 6.56 % h, 28.37% o and 8.28 % n by mass. what is the empirical formula for adrenaline
-Dominant- [34]

Answer:- An empirical formula of adrenaline is C_8H_1_1O_3N .

Solution:- Convert given percentages to moles and then calculate the mol ratio to get the simplest whole number ratio of moles of atoms which is the empirical formula of the compound.

C=\frac{56.7}{12} = 4.725 mol

H=\frac{6.56}{1} = 6.56 mol

O=\frac{28.37}{16} = 1.773 mol

N=\frac{8.28}{14} = 0.591 mol

let's calculate the mol ratio now. To calculate the mole ratio, we divide the moles of each by moleso f N as it's the least one:

C=\frac{4.725}{0.591} = 8

H=\frac{6.56}{0.591} = 11

O=\frac{1.773}{0.591} = 3

N=\frac{0.591}{0.591} = 1

So, an empirical formula of adrenaline is C_8H_1_1O_3N .


3 0
3 years ago
HELP PLEASE IM ALMOST DONE WITH CHEM FINAL AND WANT TO MAKE SURE IM DOING GOOD. PLS EXPLAIN
monitta

The Answer is "None of the Above"

6 0
2 years ago
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