Answer:
Conservative Properties of Seawater
Explanation:
The Conservative properties of seawater refer to those properties that cannot be altered due to the occurrence of physical, chemical and biological processes, over the large oceanic bodies. This typically comprises properties such as the temperature and also there is a high concentration of both sodium and chloride ions, which increases the salinity of the oceans.
These conservative properties occur in almost a fixed amount, or it most probably changes at a very slower rate through time. They can be considered to have a long residence time.
1. Increasing the temperature
The equation of line q is determined as y = ¹/₈x - ⁹/₄.
<h3>What is slope?</h3>
The slope of a line is the change in y axis to change in x axis.
<h3>Slope of line P</h3>
y = – 8x + 6
from general line equation, y = mx + c
where;
m = - 8
<h3>Slope of line q</h3>
m₂ = -1/m
m₂ = -1/-8
m₂ = 1/8
<h3>Equation of line q</h3>
(y - y₁) / (x - x₁) = m₂
(y + 2)/(x - 2) = 1/8
y + 2 = ¹/₈(x - 2)
y + 2 = ¹/₈x - ¹/₄
y = ¹/₈x - ⁹/₄
Thus, the equation of line q is determined as y = ¹/₈x - ⁹/₄.
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The molar concentration of the KI_3 solution is 0.251 mol/L.
<em>Step 1</em>. Write the <em>balanced chemical equation</em>
I_3^(-) + 2S_2O_3^(2-) → 3I^(-) + S_4O_6^(2-)
<em>Step 2</em>. Calculate the <em>moles of S_2O_3^(2-)</em>
Moles of S_2O_3^(2-)
= 27.9 mL S_2O_3^(2-) ×[0.270 mmol S_2O_3^(2-)/(1 mL S_2O_3^(2-)]
= 7.533 mmol S_2O_3^(2-)
<em>Step 3</em>. Calculate the <em>moles of I_3^(-)
</em>
Moles of I_3^(-) = 7.533 mmol S_2O_3^(2-)))) × [1 mmol I_3^(-)/(2 mmol S_2O_3^(2-)] = 3.766 mmol I_3^(-)
<em>Step 4</em>. Calculate the <em>molar concentration of the I_3^(-)
</em>
<em>c</em> = "moles"/"litres" = 3.766 mmol/15.0 mL = 0.251 mol/L
Answer:
(a) Hydrogen bonding
(b) Dispersion forces
(c) Ion-dipole forces
(d) Dipole-dipole forces
Ion-dipole forces (c) are the strongest of the 4 interactions while dispersion forces are the weakest (b).
Explanation:
The picture is missing but I think is the one that I'm uploading.
Picture (a)
HF is a polar molecule with a high difference in electronegativity between H and F. As a consequence, the force between HF molecules is Hydrogen bonding.
Picture (b)
In picture (b) we have F₂ molecules, which are nonpolar due to their atoms having the same electronegativity. The forces between nonpolar molecules are dispersion forces.
Picture (c)
Na⁺ is an ion and H₂O a dipole. Therefore, they experience ion-dipole forces.
Picture (d)
SO₂ molecules are polar, that is, they form dipoles and experience dipole-dipole forces.
Ion-dipole forces (c) are the strongest of the 4 interactions while dispersion forces are the weakest (b).
