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miss Akunina [59]
3 years ago
15

There are two steps in the usual industrial preparation of acrylic acid, the immediate precursor of several useful plastics. Cac

, (s)+2H20(I) =C,H,($) + Ca(OH),(s) 6C,H, ()+300,() + 4H2O(g) =SCH,CHCO,H (8) The net reaction is: 6 Cac,(s) +16H20 (1)+300, 6) = 6Ca(OH)($)+5CH,CHCO,H() K Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K, and Ky. If you need to include any physical constant be sure you use their standard symbols, which you'll find in the ALEKS Calculator. K-1 x 5 ?
Chemistry
1 answer:
Tanya [424]3 years ago
4 0

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

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What would be the mass of 3 moles of water molecules?
ankoles [38]

Answer:

\boxed {\boxed {\sf A. \ 54 \ grams }}

Explanation:

To convert from moles to grams, we must use the molar mass.

Recall that water's molecular formula is H₂O. It contains hydrogen and oxygen. Look up the two elements masses on the Periodic Table.

  • Hydrogen (H): 1.008 g/mol
  • Oxygen (O): 15.999 g/mol

Now, use these masses to find water's mass. The subscript of 2 tells us there are 2 atoms of hydrogen, so we multiply hydrogen's mass by 2 and add oxygen's.

  • H₂O= 2(1.008 g/mol) + 15.999 g/mol = 18.015 g/mol

Use the molar mass as a ratio.

\frac{18.015 \ g \ H_2 O}{ 1 \ mol \ H_2 O}

Multiply by the given number of moles.

3 \ mol \ H_2O*\frac{18.015 \ g \ H_2 O}{ 1 \ mol \ H_2 O}

The moles of water will cancel.

3 *\frac{18.015 \ g \ H_2 O}{ 1 }

3 *{18.015 \ g \ H_2 O}

54.045 \ g \ H_2O

Round to the nearest whole number. The 0 in the tenth place tells us to leave the number as is.

54 \ g \ H_2O

There are about <u>54 grams</u> of water in 3 moles.

7 0
3 years ago
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Choose all the correct information concerning chemical reactions: Involves small amounts of energy. Some of the mass is converte
suter [353]
<span>A chemical reactions :
Involves small amounts of energy.
</span><span> Only electrons are involved.
</span><span>The mass remains the same.</span>
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3 years ago
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Salt is ionic, and oil is covalent. If you add water, the salt will dissolve in the water, and the oil will float to the top. Yo
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Is this a question?

Cause if it is I dont understand it.

4 0
3 years ago
Given that the initial rate constant is 0.0110s−1 at an initial temperature of 21 ∘C , what would the rate constant be at a temp
gulaghasi [49]

The rate constant is mathematically given as

K2=2.67sec^{-1}

<h3>What is the Arrhenius equation?</h3>

The rate constant for a particular reaction may be calculated with the use of the Arrhenius equation. This constant can be stated in terms of two distinct temperatures, T1 and T2, as follows:

ln(\frac{K2}{K1})= (\frac{Ea}{R})*(\frac{1}{T1}-\frac{1}{T2})

Therefore

KT1= 0.0110^{-1}

T1= 21+273.15

T1= 294.15K

T2= 200  

T2=200+273.15

T2= 473.15K

Ea= 35.5 Kj/Mol

Hence, in  j/mol R Ea is

Ea=35.5*1000 j/mol R

ln(\frac{K2}{0.0110})= (\frac{35.5*1000}{8.314})*(\frac{1}{294.15}-\frac{1}{473.15}\\\\ln(\frac{K2}{0.0110})=5.492

K2/0.0110 =e^(5.492)

K2/0.0110 =242.74

K2= 242.74*0.0110

K2=2.67sec^{-1}

In conclusion, rate constant

K2=2.67sec^{-1}

Read more about rate constant

brainly.com/question/20305871

#SPJ1

5 0
2 years ago
How many moles of N are in .235g of N2O
makkiz [27]
Given the molar mass of Nitrogen is 14.01g/mol you can use that to solve for the moles of nitrogen.
0.235g(1mol/14.01g) = .0168 moles.
6 0
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