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goldfiish [28.3K]
3 years ago
5

If a temperature increase from 12.0 ∘C to 21.0 ∘C doubles the rate constant for a reaction, what is the value of the activation

barrier for the reaction
Chemistry
1 answer:
diamong [38]3 years ago
7 0

Answer:

53.7kJ/mol

Explanation:

Using Arrhenius equation

Given

T1 = 12°C = 273 + 12 = 285K

T2 = 21°C = 273 + 21 = 294K

k = A exp(-Ea/RT)

Where k = Rate constant

A = the pre-exponential factor

Ea = the activation energy

R = the Universal Gas Constant = 8.314J/kmol

T = the temperature

Taking logarithms of both sides of the Arrhenius Equation.

ln(k) = ln(A) - Ea/RT

If there are the rates at two different temperatures, we can derive the expression to be;

ln(k2/k1) = Ea/R(1/T1 - 1/T2)

The reaction doubles the rate constant

So, k2/k1 = 2 (Given)

Then we have

ln(2) = Ea/8.314(1/285 - 1/294)

ln(2) * 8.314 = Ea*(1/285 - 1/294)

6.9314E-1 * 8.314 = Ea*(1/285 - 1/294)

5.7628 = Ea*(1/285 - 1/294)

5.7628 = Ea*1.0741E-4

Ea = 5.7628 / 1.074E-4

Ea = 53657.35567970204J

Ea = 53.7kJ/mol

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In a 66.0-g aqueous solution of methanol, CH 4 O , CH4O, the mole fraction of methanol is 0.300. 0.300. What is the mass of each
Mumz [18]

Answer:

The solution is composed by 37.5 g of water and 28.5 g of methanol.

Explanation:

Total mass = 66 g

Mole fraction methanol: 0.3

Sum of mole fraction = 1

Therefore, mole fraction of water = 0.7

Let's find out the mass of each component by this two equations:

Methanol mass + Water mass = 66 g

Water mass = 66g - Methanol mass

Methanol mass = 66g - water mass

water mass / 18 g/mol = moles of water

methanol mass / 32 g/mol = moles of methanol

moles of water / total moles = 0.7

moles of methanol / total moles = 0.3

water mass / 18 g/mol / (water mass / 18 g/mol) + (methanol mass / 32 g/mol)  = 0.7 ; let's replace methanol mass, as (66 - water mass)

water mass / 18 g/mol / (water mass / 18 g/mol) + (66 - water mass / 32 g/mol)  = 0.7 → The unknown is water mass (X)

X / 18  / ( (X / 18)  + ((66-X) / 32)) = 0.7

(X / 18)  + ((66-X) / 32) = (16X + 594 - 9X)/288

X / 18  /  (16X + 594 - 9X)/288 = 0.7

X/18 = 0.7 . ( (7X + 594 ) / 288)

X / 18 = 7/2880 ( 7X + 594)

X = 7/2880 ( 7X + 594) 18

X = 7/160 (7X + 594)

X = 49/160X + 2079/80

X - 49/160X = 2079/80

111/160X = 2079/80

X = 2079/80 . 160/111 = 37.5 g → mass of water

Therefore, mass of methanol → 66 g - 37.4 g = 28.5 g

7 0
3 years ago
A particular brand of gasoline has a density of 0.737 g/ml at 25 ∘c. how many grams of this gasoline would fill a 13.0 gal tank
Usimov [2.4K]

Density of gasoline is 0.737 g/mL and volume of tank is 13.0 gal.

Since, 1 US gal=3.78 L

Volume of tank in L will be:

V=13.0 gal(\frac{3.78 L}{1 gal})=49.14 L

Also, 1 L=1000 mL

Thus,

V=49.14 L(\frac{1000 mL}{1 L})=49140 mL

Mass of gasoline can be calculated as follows:

m=d×V

Here, d is density and V is volume thus,

m=0.737 g/mL\times 49140 mL=3.62\times 10^{4}g

Therefore, mass of gasoline will be 3.62\times 10^{4}g.

7 0
3 years ago
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