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FrozenT [24]
2 years ago
15

When a bag of popcorn is opened in a room, the smell of the popcorn spreads throughout the room over time. Explain why this happ

ens using ideas about particle motion. Be specific and detailed.
Chemistry
2 answers:
KIM [24]2 years ago
7 0

Answer:

The aroma of the popcorn spreads throughout the room gradually due to the presence of air.

Explanation:

The popcorn bag releases an aroma when opened. This aroma then travels through the air due to which the aroma spreads throughout the room.

Note:

If the room was closed, the aroma will remain inside the room. If the room was open, the aroma will also spread beyond the room due to the presence of air.

Citrus2011 [14]2 years ago
6 0
Smells travel through the air by diffusion. Air particles, and the odor particles within the air, move freely in all directions plus odors are constantly moving.
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The ksp of manganese(ii) carbonate, mnco3, is 2.42 × 10-11. calculate the solubility of this compound in g/l.
Vikki [24]

Answer :  The solubility of this compound in g/L is 565.414\times 10^{-6}g/L.

Solution : Given,

K_{sp}=2.42\times 10^{-11}

Molar mass of MnCO_3 = 114.945g/mole

The balanced equilibrium reaction is,

                      MnCO_3\rightleftharpoons Mn^{2+}+CO^{2-}_3

At equilibrium                         s       s

The expression for solubility constant is,

K_{sp}=[Mn^{2+}][CO^{2-}_3]

Now put the given values in this expression, we get

2.42\times 10^{-11}=(s)(s)\\2.42\times 10^{-11}=s^2\\s=0.4919\times 10^{-5}=4.919\times 10^{-6}moles/L

The value of 's' is the molar concentration of manganese ion and carbonate ion.

Now we have to calculate the solubility in terms of g/L multiplying by the Molar mass of the given compound.

s=4.919\times 10^{-6}moles/L\times 114.945g/mole=565.414\times 10^{-6}g/L

Therefore, the solubility of this compound in g/L is 565.414\times 10^{-6}g/L.


8 0
2 years ago
An unknown acid solution has PH 3.4. 66% of the acid is ionized. Whats the pka?
juin [17]

Answer:

pKa=3.58

Explanation:

Hello,

In this case, since the pH defines the concentration of hydrogen:

pH=-log([H^+])

[H^+]=10^{-pH}=10^{-3.4}=3.98x10^{-4}

And the percent ionization is:

\% \ ionization=\frac{[H^+]}{[HA]}*100\%

We compute the concentration of the acid, HA:

[HA]=\frac{[H^+]}{\% \ ionization}*100\%=\frac{3.98x10^{-4}}{66\%}  *100\%\\\\

[HA]=6.03x10^{-4}

Thus, the Ka is:

Ka=\frac{[H^+][A^-]}{[HA]}=\frac{3.98x10^{-4}*3.98x10^{-4}}{6.03x10^{-4}}\\  \\Ka=2.63x10^{-4}

So the pKa is:

pKa=-log(Ka)=-log(2.63x10^{-4})\\\\pKa=3.58

Regards.

5 0
2 years ago
What does it mean to say that the electric current from a wall socket is “120 V AC”?
patriot [66]
I don't know what you are asking but AC= Alternative current
V= Volt
5 0
2 years ago
What would happen if you play a note in a cold day on a flute?
Maurinko [17]
I don't know if this is the answer you are looking for but it would be flat unless the player pushed the tuning slide in.
7 0
3 years ago
How many milligrams of magnesium reacts with excess HCl to produce 31.2 mL of hydrogen gas at 754 Torr and 25.0℃.
Ivanshal [37]

Answer:

There will react 30.9 milligrams of magnesium

Explanation:

Step 1: Data given

Volume of hydrogen = 31.2 mL

Pressure = 754 torr = 754/760 = 0.992 atm

Temperature = 25.0 °C = 298 Kelvin

Step 2: The balanced equation

Mg + 2HCl → MgCl2 + H2

Step 3: Calculate moles of H2

p*V = n*R*T

⇒ with p = the pressure of H2 = 0.992 atm

⇒with V = the volume of H2 = 31.2 mL = 0.0312 L

⇒ with n = the moles of H2 = TO BE DETERMINED

⇒ with R = the gas constant = 0.08206 L*atm/K*mol

⇒ with T= the temperature = 25.0 °C = 298 Kelvin

n = (p*V)/(R*T)

n = (0.992*0.0312)/(0.08206*298)

n = 0.00127 moles

Step 4: Calculate moles of Mg

For 1 mol of Mg we need 2 moles of HCl to produce 1 mol of MgCl2 and 1 mol of H2

For 0.00127 moles of H2 we need 0.00127 moles of Mg

Step 5: Calculate mass of Mg

Mass of Mg = moles of Mg * molar mass of Mg

Mass of Mg = 0.00127 moles * 24.3 g/mol

Mass of Mg = 0.0309 grams = 30.9 mg of Mg

There will react 30.9 milligrams of magnesium

3 0
2 years ago
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