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creativ13 [48]
2 years ago
12

11. Which of the following best explains why Co, gas is easily compressible but solid CO, (dry ice) is incompressible?​

Chemistry
1 answer:
telo118 [61]2 years ago
4 0

Answer:

The molecules of solid CO2 are much closer together than the molecules of CO2 gas.

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In the formation of a solution how does the solvent differ from the solute
dlinn [17]
Solute is a substance that dissolves in a solvent in order to form a solution. Solutes can be in liquid, gaseous or solid phase. Normally, in a solution, solutes are in a lesser amount than the solvents. When a solution has the maximum amount of solutes it can dissolve, then the solution is said to be saturated.
6 0
3 years ago
10. At 573K, NO2(g) decomposes forming NO and O2. The decomposition reaction is second order in NO2 with a rate constant of 1.1
leva [86]

Answer:

48.67 seconds

Explanation:

From;

1/[A] = kt + 1/[A]o

[A] = concentration at time t

t= time taken

k= rate constant

[A]o = initial concentration

Since [A] =[A]o - 0.75[A]o

[A] = 0.056 M - 0.042 M

[A] = 0.014 M

1/0.014 = (1.1t) + 1/0.056

71.4 - 17.86 = 1.1t

53.54 = 1.1t

t= 53.54/1.1

t= 48.67 seconds

Hence,it takes 48.67 seconds to decompose.

6 0
2 years ago
How many helium atoms are there in a helium blimp containing 539kg of helium
MaRussiya [10]
Atomic mass of helium is 4.002642g/mol 
(542000g)/(4.002642g/mol)*6.02*10^23 = 8.15*10^28 atoms
3 0
2 years ago
Read 2 more answers
Help! I am in a hurry! Will get brainliest if correct!
sashaice [31]

Answer:

nonmetel

Explanation:

3 0
3 years ago
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The average atomic weight of copper, which has two naturally occurring isotopes, is 63.5. One of the isotopes has an atomic weig
Darya [45]

<u>Answer:</u> The atomic weight of the second isotope is 64.81 amu.

<u>Explanation:</u>

Average atomic mass of an element is defined as the sum of atomic masses of each isotope each multiplied by their natural fractional abundance

Formula used to calculate average atomic mass follows:

\text{Average atomic mass }=\sum_{i=1}^n\text{(Atomic mass of an isotopes)}_i\times \text{(Fractional abundance})_i     .....(1)

We are given:

Let the mass of isotope 2 be 'x'

Mass of isotope 1 = 62.9 amu

Percentage abundance of isotope 1 = 69.1 %

Fractional abundance of isotope 1 = 0.691

Mass of isotope 2 = 'x'

Percentage abundance of isotope 2 = 30.9%

Fractional abundance of isotope 2 = 0.309

Average atomic mass of copper = 63.5 amu

Putting values in equation 1, we get:

\text{Average atomic mass of copper}=[(62.9\times 0.691)+(x\times 0.309)]

x=64.81amu

Hence, the atomic weight of second isotope will be 64.81 amu.

4 0
2 years ago
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