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3 years ago

Under which of the following sets of conditions would the most o2 (g) be dissolved in h2o(l)?

Chemistry

1 answer:

jek_recluse [69]3 years ago

6 0

Answer:

Oxygen will dissolve more in H2O at 5 atm and 20 °C than at 5 atm 80 °C

Option B is correct.

Explanation:

Step 1: Data given

Pressure = 5 atm

Temperature = 20 °C or 80 °C

Step 2:

At low pressure, a gas has a low solubility. Decreased pressure allows more gas molecules to be present in the air, with very little being dissolved in solution. At high(er) pressure, a gas has a high solubility.

This means the higher the pressure the more the gas will dissolve. Since The pressure stays constant, it depends on the temperature.

The solubility of gases in liquids decreases with increasing temperature.

This means the gas will dissolve more with a lower temperature.

Oxygen will dissolve more in H2O at 5 atm and 20 °C than at 5 atm 80 °C

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A freezer compartment is covered with a 2-mm-thick layer of frost at the time it malfunctions. If the compartment is in ambient

ruslelena [56]

Answer:

The time required to melt the frost is 3.25 hours.

Explanation:

The time required to melt the frost dependes on the latent heat of the frost and the amount of heat it is transfered by convection to the air .

The heat transferred per unit area can be expressed as:

$q=h_c*A*\Delta T\\\\q/A=h_c*\Delta T$

being hc the convective heat transfer coefficient (2 Wm^-2K^-1) and ΔT the difference of temperature (20-0=20 °C or K).

$q/A=h_c*\Delta T=2\frac{W}{m^2K}*20K=40\frac{W}{m^2}$

If we take 1 m^2 of ice, with 2 mm of thickness, we have this volume

$V=T*A = 0.002 m * 1 m^2=0.002m^3$

The mass of the frost can be estimated as

$M=\rho * V=700\frac{kg}{m^3}*0.002m^3= 1.4 kg$

Then, the amount of heat needed to melt this surface (1 m²) of frost is

$Q=L*M=334\frac{kJ}{kg}*1.4kg= 467.6kJ$

The time needed to melt the frost can be calculated as

$t=\frac{Q}{(q/A)}=\frac{467.6kJ/m2}{40W/m2} = 11.69\frac{kJ}{W}*\frac{1W*s}{1J}*\frac{1000J}{1kJ}= 11690s=3.25h$

7 0

3 years ago

How many moles of KBr will be produced from 10.51 moles of BaBr2?

gregori [183]

Answer:

21.02moles of KBr

Explanation:

Parameters given:

Number of moles BaBr₂ = 10.51moles

Complete reaction equation:

BaBr₂ + K₂SO₄ → KBr + BaSO₄

Upon inspecting the given equation, we find out that the atoms are not balanced on both sides of the equation:

The balanced equation is:

BaBr₂ + K₂SO₄ → 2KBr + BaSO₄

From the equation:

1 mole of BaBr₂ produces 2 moles of KBr

∴ 10.51 moles of BaBr₂ will yield (2 x 10.51) moles = 21.02moles of KBr

7 0

3 years ago

All atoms of a given element are identical was proven wrong because of the existence or

vagabundo [1.1K]

Answer:

they are all similar

Explanation:

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3 years ago

Which of the following instruments is a combination of a percussion and a stringed instrument?

murzikaleks [220]

Answer:B

Explanation:

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3 years ago

Which of the following is non polar covalent bond?

vladimir2022 [97]

Answer:

N-Cl

Explanation:

Look at the chart below. Since N-Cl bond has a electronegativity difference of (3.0-3.0) zero, they are non-polar.

5 0

2 years ago