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3 years ago

Is oxygen soluble in water

Chemistry

2 answers:

s2008m [1.1K]3 years ago

7 0

Answer: Yes

Explanation:

Oxygen is relatively insoluble in water, its solubility being only 264 µM at 25 °C. That explains in part why you (and fish) require dedicated oxygen carriers in your blood to transfer sufficient oxygen around your body.

telo118 [61]3 years ago

4 0

Answer:

Oxygen is relatively insoluble in water

Explanation:

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A reaction has ?h?rxn= -129 kj and ?s?rxn= 301 j/k .

Gennadij [26K]

I was thinking that the question would be to find for the operating temperature of the reaction. Change in entropy is equal to the total energy divided by the temperature. Assuming it is isothermal, internal energy would be zero. Therefore, the temperature would be:

T = 129000/301 = 428.57 K

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4 years ago

Phosphorus has five valence electrons and hydrogen has one valence electron. What would be the Lewis dot (electron dot) structur

Liula [17]

PH3 looks just like ammonia NH3 with a lone pair and 3 hydrogens in a pyramidal formation.

In PH3 the P has 3 bond pairs and 1 lone pair, (4 total pairs). The shape is called trigonal pyramidal (approximately tetrahedral minus one atom).

I hope my answer has come to your help. Thank you for posting your question here in Brainly. We hope to answer more of your questions and inquiries soon. Have a nice day ahead!

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3 years ago

Read 2 more answers

If 1.00 mol of argon is placed in a 0.500-L container at 27.0 degree C , what is the difference between the ideal pressure (as p

ElenaW [278]

Answer:

2.0 atm is the difference between the ideal pressure and the real pressure.

Explanation:

If 1.00 mole of argon is placed in a 0.500-L container at 27.0 °C

Moles of argon = n = 1.00 mol

Volume of the container,V = 0.500 L

Ideal pressure of the gas = P

Temperature of the gas,T = 27 °C = 300.15 K[/tex]

Using ideal gas equation:

$PV=nRT$

$P=\frac{1.00 mol\times 0.0821 L atm/mol K\times 300.15 K}{0.500 L}=49.28 atm$

Vander wall's of equation of gases:

The real pressure of the gas= $p_v$

For argon:

$a=1.345 L^2 atm/mol^2$

b=0.03219 L/mol.

$(p_v+(\frac{an^2}{V^2})(V-nb)=nRT$

$(p_v+(\frac{(1.345 L^2 atm/mol^2)\times (1.00 mol)^2}{(0.500 L)^2})(0.500 L-1.00 mol\times 0.03219L/mol)=1.00 mol\times 0.0821 L atm/mol K\times 300.15 K$

$p_v = 47.29 atm$

Difference : $p - p_v= 49.28 atm - 47.29 atm = 1.99 atm\approx 2.0 atm$

2.0 atm is the difference between the ideal pressure and the real pressure.

6 0

3 years ago

In the box next to your answer.

ch4aika [34]

Answer:

D equal numbers of protons and electrons

Explanation:

An atom of an element will always contain equal number of protons and electrons.

Atoms are electrically neutral because the number of positive charges and negative charges within them are always equal.

An atom is the smallest indivisible particles of an element that takes part in a chemical reaction.
The positively charged particles within an atom are the protons.
The negatively charged particles within an atom are the electrons.

For;

So number of protons = number of electrons within an atom.

6 0

3 years ago

Calculate the volume of a 2.30 mol/L solution of Na2CO3 that contains 0.325 mol of solute.

Blababa [14]

Answer:

141 mL is the volume of a 2.30 mol/L solution of Na₂CO₃ that contains 0.325 mol of solute.

Explanation:

Molarity is a measure of concentration of a solution that indicates the amount of moles of solute that appear dissolved in each liter of the mixture.

So 2.30 mol / L indicates that 2.30 moles dissolve in 1 L of solution. You want to know in what volume is contained 0.325 mol of solute. For this you apply the following rule of three: if 2.30 moles of solute are present in 1 L of solution, 0.325 moles in how much volume is it?

$volume=\frac{0.325 moles*1L}{2.30 moles}$

volume= 0.141 L

Being 1L=1000 mL, then 0.141 L=141 mL

141 mL is the volume of a 2.30 mol/L solution of Na₂CO₃ that contains 0.325 mol of solute.

5 0

3 years ago