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3 years ago

What is the volume of 0.200 mol of an ideal gas at 200 kPa and 400 K? A. 0.83 L B. 3.33 L C. 5.60 L D. 20.8 L

2 answers:

7 0

The ideal gas under STP is 22.4 L/mol. While the gas has a rule of P1V1/T1=P2V2/T2.
So the volume under 101 kPa and 273 K is 0.2*22.4=4.48 L.
So under 200 kPa and 400 K is 3.33 L. So the answer is B.

amid [387]3 years ago

3 0

Since it is stated that it is an ideal gas, we use the ideal gas equation to solve the volume of this gas sample. The ideal gas equation is expressed as:

PV = nRT
V = nRT / P
V = 0.200 (8.314) (400) / 200x10^3
V = 3.33 x 10^-3 m³ or 3.33L

Therefore, the correct answer is option B.

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A solution contains 42.0 g of heptane (C7H16) and 50.5 g of octane (C8H18) at 25 ∘C. The vapor pressures of pure heptane and pur

Kruka [31]

Answer:

(a) 22.3 torr; 5.6 torr; (b) 27.9 torr; (c) 77.7 % heptane; 23.3 % octane

(d) Heptane is more volatile than octane

Explanation:

We can use Raoult's Law to solve this problem.

It states that the partial pressure of each component of an ideal mixture of liquids is equal to the vapour pressure of the pure component multiplied by its mole fraction. In symbols,

$p_{i} = \chi_{i} p_{i}^{\circ}$

(a) Vapour pressure of each component

Let heptane be Component 1 and octane be Component 2.

(i) Moles of each component

$n_{1} = \text{42.0 g} \times \dfrac{\text{1 mol}}{\text{100.20 g}} = \text{0.4192 mol}\\n_{2} = \text{50.5 g} \times \dfrac{\text{1 mol}}{\text{114.23 g}} = \text{0.4421 mol}$

(ii) Total moles

$n_{\text{tot}} = 0.4192 + 0.4421 = \text{0.8613 mol}$

(iiii) Mole fractions of each component

$p_{1} = 0.4867 \times 45.8 = \textbf{22.3 torr}\\p_{2} = 0.5133 \times 10.9 = \ \textbf{5.6 torr}$

(iv) Partial vapour pressures of each component

$p_{1} = 0.4867 \times 45.8 = \textbf{22.3 torr}\\p_{2} = 0.5133 \times 10.9 = \textbf{5.6 torr}$

(b) Total pressure

$p_{\text{tot}} = p_{1} + p_{2} = 22.3 + 5.6 = \text{27.9 torr}$

(c) Mass percent of each component in vapour

$\chi_{1} = \dfrac{p_{1}}{p_{\text{Tot}}} = \dfrac{22.3}{27.9} =0.799\\\chi_{2} = \dfrac{p_{2}}{p_{\text{Tot}} }= \dfrac{5.6}{27. 9} =0.201$

The ratio of the mole fractions is the same as the ratio of the moles.

$\dfrac{n_{1}}{n_{2}} = \dfrac{0.799}{0.201}$

If we have 1 mol of vapour, we have 0.799 mol of heptane and 0.201 mol of octane

$m_{1} = 0.799 \times 100.20 = \text{80.1 g}\\m_{2} = 0.201\times 114.23 = \text{23.0 g}\\m_{\text{tot}} = 80.1 + 23.0 = \text{103.1 g}\\\\\text{ mass percent heptane} = \dfrac{80.1}{103.1} \times 100 \, \% = \mathbf{77.7\, \%}\\\\\text{ mass percent octane} = \dfrac{23.0}{103.1} \times 100 \, \% = \mathbf{22.3\, \%}}$

(d) Enrichment of vapour

The vapour is enriched in heptane because heptane is more volatile than octane.

5 0

3 years ago

omplete the relationship between ph and pka for each of the following atomic view pictures of a buffered solution.

Yakvenalex [24]

The relationship between pH and pKa of buffer solution in given atomic view:

In figure I pH= pKa ( since [HA] =[A-] )

In figure II pH > pKa ( since [A-] > [HA] )

In figure III pH < pKa ( since [A-] < [HA] )

The pH and pKa are related by the Henderson-Hasselbalch equation. It should not be used for concentrated solutions, extremely low pH acids, or extremely high pH bases because it is simply an approximation.

pH = pKa + log(conjugate base/weak acid).

pH equals pKa plus log ([A-] / [HA]).

pH is determined by dividing the weak acid concentration by the log of the conjugate base concentration and the pKa value.

About halfway to the equivalence point:

pH = pKa

It's important to note that this equation is familiar with the connection because it is sometimes written for the Ka value rather than the pKa value.

pKa = – log Ka

Hence, value of pH depend on relative concentration of [A-] and HA]

To know more about Ka.

brainly.com/question/16035742

#SPJ4

5 0

1 year ago

Describe the electron distribution in a polar-covalent bond and it's effect on the partial charges of the compound?

Artemon [7]

Answer:

In polar Covalent bonds, the electrons which are in bonded shifts towards an atom which has more valance electrons.

Explanation:

We know if an atom takes the electron it acquires a negative charge whereas if it gives an electron it acquires a positive charge in the ionic bond. But here we are talking about covalent bonds. Covalent bonds are those in which atoms share the electron instead of completely giving off the electron. If the atoms are identical in case of covalent bond that is 2 hydrogen atoms then this type of bonding is called pure covalent bonds but if the atoms linked in covalent bonds are different then it is called polar covalent bonds.

In this, the bonding electrons will shift towards an atom which has more valence electron thereby acquiring the partial negative charges and the other atom will acquire a partial positive charge. For example, HCl. In this the Chlorine atom is having more valence electron than hydrogen atom, and hence Chlorine atom has a partial negative charge and Hydrogen atom has a partial positive charge.

5 0

3 years ago

What is the mass of solute dissolved in 50,0 g of 12.5% saline solution? A) 7.148 B) 6.258 C) 43.88 D) 4.00 g

Marizza181 [45]

Answer:

6.25 grams is the mass of solute dissolved.

Explanation:

w/w % : The percentage mass or fraction of mass of the of solute present in total mass of the solution.

$w/w\%=\frac{\text{Mass of solute}}{\text{Mass of solution}}\times 100$