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3 years ago

The elementary reversible reaction:

Chemistry

1 answer:

serious [3.7K]3 years ago

6 0

Answer:

$Kc=0.9375$

Explanation:

Hello,

In this case, considering that A's initial concentration is 4.0mol/dm³, considering the equilibrium conversion, one obtains for the equilibrium:

$C_A^{eq}=4.0mol/dm^3*(1-x_{eq})=4.0mol/dm^3*(1-0.6)=1.6mol/dm^3\\C_B^{eq}=4.0mol/dm^3*x_{eq}=2.4mol/dm^3$

Thus, the equilibrium constant turns out:

$Kc=\frac{C_B}{C_A^2} =\frac{2.4}{1.6^2}=0.9375$

Best regards.

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Vlad1618 [11]

Answer:

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Explanation:

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3 years ago

A solution is 5.00% potassium chloride by mass. How much potassium chloride would you expect to collect by evaporating 150.0 g o

stepan [7]

Answer:

C. 7.50g

Explanation:

The percent (%) by mass of a solute in a solution refers to the number of grams contained in 100g of solution by that solute. In this case, 5% by mass of pottasium chloride (KCl) means 5g of KCl is contained in 100g of solution.

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5g/100g × 150g

= 0.05 × 150

= 7.50g of KCl solute.

Hence, 7.50g of pottasium chloride would be expected to be collected by evaporating 150.0 g of the solution.

8 0

3 years ago

4. A piece of metal weighing 0.0713 g was placed in a eudiometer containing dilute aqueous HCl. After the metal fully dissolved,

Anastasy [175]

Complete Question

4. A piece of metal weighing 0.0713 g was placed in a eudiometer containing dilute aqueous HCl. After the metal fully dissolved, 23.5 mL of hydrogen gas was collected by displace-ment of water and a 400 mm column of water was observed. The water temperature was 258C and the barometric pressure was 758.8 mm Hg (torr). Refer to the Introduction and data sheet to solve the following problems.

a) What is the vapor pressure of the water vapor in the column? (Consult Appendix E.)

b) What is the pressure of the water column expressed in mm Hg (torr)? The density of mercury is 13.6 g/mL.

c) Calculate the pressure of the hydrogen gas above the water in the column.

d) Calculate the volume occupied by the hydrogen gas at STP.

Answer:

a) $25\textdegree C=23.8 torrs$

b) $P_w=758.8$

c) $P_w=758.8=735torr$

d) $V_2=20.82mL$

Explanation:

From the question we are told that:

Metal weight $M_m=0.0713g$

Volume Hydrogen $V_h=23.5mL$

Displace-ment Column of water 400 mm column of water

Temperature $T =258\textdegree C$

Barometric Pressure $p=758.8mmHg$

Vapour Pressure of water at $25^oC$

Generally from (Consult Appendix E.)

Va-pour Pressure of water at

$25\textdegree C=23.8 torrs$

Pressure of Water column

$P_w=758.8$

c) Pressure of Water column (Consult Appendix E.)

$P_w=758.8=735torr$

Generally the equation for ideal gas is mathematically given by

$\frac{p_1v_1}{T_1}=\frac{p_2v_2}{T_2}$

Therefore

$V_2=\frac{p_1V_1T_2}{T_1p_2}$

$V_2=\frac{735*23.5*273}{298*760}$

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5 0

3 years ago

A 10.0-gram sample of which element has the smallest volume at STP?

DaniilM [7]

(4) zinc

Explanation:

Given parameters:

Mass of the sample = 10g

Condition = STP

Unknown:

Element with the least volume = ?

Solution:

The number of moles of substance as STP can be derived using the equation below;

Volume of substance = number of moles x 22.4

Number of moles = $\frac{mass}{molar mass}$

since mass = 10g

Number of moles of Al = $\frac{10}{27}$ = 0.37mole

Number of moles of Ti = $\frac{10}{47.9}$ = 0.29mole

number of moles of Mg = $\frac{10}{24}$ = 0.47mole

Number of moles of Zn = $\frac{10}{65.5}$ = 0.15mole

Zinc has the least number moles and it will have the lowest volume at STP because the volume directly proportional to number of moles.

learn more:

Number of moles brainly.com/question/1841136

#learnwithBrainly

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4 years ago

How many moles is in 2.52*10^24 molecules of water?

nataly862011 [7]

Hi friend
--------------
Your answer
-------------------

Water = H2O

Number of molecules in one mole of water = 6.022 × 10²³ [Avogadro's constant]

Given number of molecules = 2.52 × 10²³

So,
------

Number of moles =
$\frac{2.52 \times 10 {}^{24} }{6.022 \times 10 {}^{23} } \\ \\ = 4.184 \: (approximately)$

HOPE IT HELPS

3 0

3 years ago