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2 years ago

How many moles are in 1.84x10^24 formula units of CaCl2, calcium chloride?

1 answer:

7 0

1 mole = 6.022 * 10^23 formula units.

1.84*10^24 formula units CaCl₂ * (1 mole CaCl₂/6.022*10^23 formula units CaCl₂) = 3.06 moles of CaCl₂.

There are 3.06 moles of CaCl₂.

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Answer:

The equation that gives the overall equilibrium in terms of the equilibrium constants K and Ky is K1 = K^6 * Ky

Explanation:

we have the following balanced reaction:

CaC2 + 2H2O = C2H2 + Ca(OH)2

the value of K for this reaction will be equal to:

K = ([C2H2] * [Ca(OH)2])/([CaC2] * [H2O]^2)

if we multiply the reaction by the value of 6, we have:

6CaC2 + 12H2O = 6C2H2 + 6Ca(OH)2

Again, the value of K for this reaction will be equal to:

K,´ = ([C2H2] ^6 * [Ca(OH)2]^6)/([CaC2]^6 * [H2O]^12) = K^6

For the second reaction:

6C2H2 + 3CO2 + 4H2O = 5CH2CHCO2H

The value of K for this reaction:

K2 = ([CH2CHCO2H]^5)/([C2H2]^6 * [CO2]^3 * [H2O]^4)

we also have:

K1 = ([CH2CHCO2H]^5)/([C2H2]^6 * [CO2]^3 * [H2O]^16)

Thus:

K1 = K^6 * Ky

4 0

2 years ago

How many molecules of carbon dioxide are dissolved in 0.550 L of water at 25 °C if the pressure of CO2 above the water is 0.250

Grace [21]

Answer: The number of molecules of carbon dioxide gas are $2.815\times 10^{21}$

Explanation:

To calculate the molar solubility, we use the equation given by Henry's law, which is:

$C_{CO_2}=K_H\times p_{CO_2}$

where,

$K_H$ = Henry's constant = $0.034mol/L.atm$

$C_{CO_2}$ = molar solubility of carbon dioxide gas

$p_{CO_2}$ = pressure of carbon dioxide gas = 0.250 atm

Putting values in above equation, we get:

$C_{CO_2}=0.034mol/L.atm\times 0.250atm\\\\C_{CO_2}=8.5\times 10^{-3}M$

To calculate the number of moles for given molarity, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}$

Molarity of carbon dioxide = $8.5\times 10^{-5}M$

Volume of solution = 0.550 L

Putting values in above equation, we get:

$8.5\times 10^{-3}M=\frac{\text{Moles of }CO_2}{0.550L}\\\\\text{Moles of }CO_2=(8.5\times 10^{-3}mol/L\times 0.550L)=4.675\times 10^{-3}mol$

According to mole concept:

1 mole of a compound contains $6.022\times 10^{23}$ number of molecules

So, $4.675\times 10^{-3}$ moles of carbon dioxide will contain = $(6.022\times 10^{23}\times 4.675\times 10^{-3})=2.815\times 10^{21}$ number of molecules