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tino4ka555 [31]
3 years ago
12

You find small pieces of ice instead of ice cubes in the freezer. State how this is possible.

Chemistry
1 answer:
Nat2105 [25]3 years ago
4 0
Well, if u had a spilled liquid in there (we'll simply go with water) and you had the freezer at a cold temperature it would change (like,icycles on trees when it's snowing)
You might be interested in
Methanethiol, CH3SH, has a substantial dipole mement (1.52) even though carbon and sulfer have identical electronegativities. Ex
AleksAgata [21]

Answer:

The whole molecule is polar because Sulfur has lone pairs but Carbon doesn't. Lone pairs count more toward polarity, shifting dipole toward S.

Explanation:

Even though carbon and sulfur have identical values of electronegativities, the molecule, CH_3SH is polar because of the presence of the lone pairs on the sulfur atom.

The C-S bond is not polar because the both the atoms have electronegatiivty. <u>But S has lone pairs which can attract the bond pairs of the bond between the S and H and thus acquires slightly negative charge and H acquires slightly positive charge.</u>

6 0
3 years ago
Iridium has two naturally occurring isotopes, Iridium-191 and Iridium-193. If the average atomic mass of orodum s 192.217, what
Lina20 [59]

Answer:

The percent isotopic abundance of Ir-193 is 60.85 %

The percent isotopic abundance of Ir-191 is 39.15 %

Explanation:

we know there are two naturally occurring isotopes of iridium, Ir-191 and Ir-193

First of all we will set the fraction for both isotopes

X for the isotopes having mass 193

1-x for isotopes having mass 191

The average atomic mass is 192.217

we will use the following equation,

193x + 191(1-x) = 192.217

193x + 191 - 191x = 192.217

193x- 191x = 192.217 - 191

2x = 1.217

x= 1.217/2

x= 0.6085

0.6085 × 100 = 60.85 %

60.85% is abundance of Ir-193 because we solve the fraction x.

now we will calculate the abundance of Ir-191.

(1-x)

1-0.6085 =0.3915

0.3915× 100= 39.15 %

6 0
3 years ago
How many moles of 02 can be prepared from 6.75 moles of KCIO3 ?
Varvara68 [4.7K]

The equation for this question could be 2KClO_{3}→2KCl+3O_{2} .

so for 6.75 moles of KClO_{3}  *3 moles of O_{2}/2 moles of KClO_{3}

= 10.125

5 0
3 years ago
7. Lawrencium has a half-life of 3.00 minutes. I started with a 100.0 g sample. After 45.0 minutes how
Zinaida [17]

Answer:

N=3.05*10^-3g

Explanation:

Using Ln(No/N)=0.693/t½*t

Ln(No/N)=0.693/3*45

No/N=exp(10.396)

100/exp(10.396)=N

100/32695.7=N

N=3.05*10^-3g

6 0
3 years ago
An acetate buffer solution is prepared by combining 50. mL of a 0.20 M acetic acid, HC2H3O2 (aq), and 50. mL of 0.20 M sodium ac
Gala2k [10]

Answer:

B. CH3COOH pH > 4.7 (4.8)

Explanation:

  • CH3COOH + NaOH ↔ CH3COONa + H2O
  • CH3COONa + NaOH ↔ CH3COONa

∴ mol NaOH = (5 E-3 L)*(0.10 mol/L) = 5 E-4 mol

⇒ mol CH3COOH = (0.05 L)*(0.20 mol/L) = 0.01 mol

⇒ <em>C</em> CH3COOH = (0.01 mol - 5 E-4 mol) / (0.105 L)

⇒ <em>C</em> CH3COOH = 0.0905 M

∴ mol CH3COONa = (0.05 L )*(0.20 mol/L) = 0.01 mol

⇒ <em>C</em> CH3COONa =  (0.01 mol + 5 E-4 mol) / (0.105 L )

⇒ <em>C</em> CH3COONa = 0.1 M

∴ Ka = ([H3O+]*(0.1 + [H3O+])) / (0.0905 - [H3O+]) = 1.75 E-5

⇒ 0.1[H3O+] + [H3O+]² = (1.75 E-5)*(0.0905 - [H3O+])

⇒ [H3O+]² 0.1[H3O+] = 1.584 E-6 - 1.75 E-5[H3O+]

⇒ [H3O+]² + 0.1000175[H3O+] - 1.584 E-6 = 0

⇒ [H3O+] = 1.5835 E-5 M

∴ pH = - Log [H3O+]

⇒ pH = - Log (1.5835 E-5)

⇒ pH = 4.8004 > 4.7

7 0
3 years ago
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