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3 years ago

When two clear substance combines, an insoluble solid is formed that settle downs as a

Chemistry

1 answer:

FinnZ [79.3K]3 years ago

7 0

$\huge \sf \underline \blue{Question} \colon$

When two clear substance combines, an insoluble solid is formed that settle downs as a ________.

$\huge \sf \underline \blue{Answer} \colon$

When two clear substance combines, an insoluble solid is formed that settle downs as a precipitate.

→A precipitate is a substance to be deposited in solid form from a solution.

______________________________________

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You find a mysterious bottle in the laboratory labeled 0.01 M Sodium Hydroxide. What is the pH of the solution?

andrey2020 [161]

Answer: pH of the solution is 12

Explanation:

NaOH —> Na+ + OH-

NaOH = 0.01M

Na+ = 0.01M

OH- = 0.01M

pOH = —log [OH-] = —log [0.01]

pOH = 2

pH + pOH = 14

pH = 14 — pOH = 14 — 2 = 12

pH = 12

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4 years ago

It takes 330 j of energy to raise the temperature of 14.6 g of benzene from 21.0 °c to 28.7 °c at constant pressure. What is the

Akimi4 [234]

The mathematical expression for heat capacity at constant pressure is given as:

$Q=n\times C_{p}\times \Delta T$ (1)

where, Q = heat capacity

$C_{p}$ = molar heat capacity at constant pressure

$\Delta T$ = change in temperature

n = number of moles

Therefore, $\Delta T$ = $28.7^{o}C-21^{o}C$

= $7.7 ^{o}C$

Number of moles = $\frac{given mass in g}{molar mass}$

= $\frac{14.6 g }{78.11 g/mol}$

= 0.186 mole

Put the values in formula (1)

$330 J=0.186 mole\times C_{p}\times (7.7 ^{o}C+ 273)$ (conversion of degree Celsius into kelvin)

$C_{p} = \frac{330 J}{0.186 mole\times 280.7 K}$

= $\frac{330 J}{52.2102 mole K}$

= 6.32 J /mol K

Hence, molar heat capacity of benzene at constant pressure = $6.32 Jmol^{-1} K^{-1}$

6 0

4 years ago

Atoms of elements at the top of a group on the periodic table are smaller than the atoms of elements at the bottom of the group.

Serjik [45]

I think the correct answer would be the last one.

7 0

3 years ago

Read 2 more answers

How much heat is required to take a 150 g sample of water from 10.0 ℃ to 95.0 ℃? cs,water = 4.184 J/g*℃

Setler79 [48]

Answer:

$\boxed {\boxed {\sf 53, 346 \ Joules}}$

Explanation:

We are given the specific heat and change in temperature, so we should use this heat formula:

$q=m C \Delta T$

where m is the mass, C is the specific heat capacity, and ΔT is the change in temperature.

We know the mass is 150 grams. The specific heat of water is 4.184 J/g °C.

Let's find the change in temperature.

Subtract the initial temperature from the final temperature.

ΔT= final temp - initial temp
final= 95.0 °C and initial= 10.0 °C
ΔT= 95.0 °C - 10.0 °C= 85.0 °C

Now we know all the values:

$m= 150 \ g \\C= 4.184 J/ g \ \textdegree C \\\Delta T= 85.0 \textdegree C$

Substitute them into the formula.

$q=(150 \ g) (4.184 \ J/g \ \textdegree C)(85.0 \textdegree C )$

Multiply all three numbers together. Note that the grams (g) and degrees Celsius (°C) will cancel out. Joules (J) will be the only remaining unit.

$q=(627.6 \ J/ \textdegree C) ( 85.0 \textdegree C)$

$q=53346 \ J$

53,346 Joules of heat are required.

4 0

3 years ago

How many atoms are present in 354.22 g of cl2

Valentin [98]

Answer:

a) 3.0076 E24 atoms

Explanation:

mol ≡ 6.022 E23 atoms

∴ mass Cl2 = 354.22 g

∴ molar mass Cl2 = 70.906 g/mol

⇒ mol Cl2 = (354.22 g)*(mol/70.906 g) = 4.9956 mol

⇒ atoms Cl2 = (4.9956 mol)*(6.022 E23 atoms/mol)

⇒ atoms Cl2 = 3.008 E24 atoms

3 0

3 years ago