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kaheart [24]
3 years ago
12

The half-life of a first-order reaction is 13 min. If the initial concentration of reactant is 0.085 M, how long would it take u

ntil the concentration decreases to 0.055 M
Chemistry
1 answer:
olasank [31]3 years ago
5 0

Answer: It will take 8.2 minutes until the concentration decreases to 0.055 M

Explanation:

The time after which 99.9% reactions gets completed is 40 minutes

Explanation:

Expression for rate law for first order kinetics is given by:

t=\frac{2.303}{k}\log\frac{a}{a-x}

where,

k = rate constant

t = age of sample

a = let initial amount of the reactant

a - x = amount left after decay process  

a) for completion of half life:

Half life is the amount of time taken by a radioactive material to decay to half of its original value.

t_{\frac{1}{2}}=\frac{0.693}{k}

k=\frac{0.693}{13min}=0.053min^{-1}

b)  Time taken for 0.085 M to decrease to 0.055 M

t=\frac{2.303}{0.053}\log\frac{0.085}{0.055}

t=8.2min

Thus it will take 8.2 minutes until the concentration decreases to 0.055 M

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Sedaia [141]
1 mole = 6.022×10^23 atoms. 1 water molecule = 2 Hydrogen atoms + 1 oxygen atom. So, 1 mole H2O = 1.2044×10^24 hydrogen atoms. Therefore 2 mole H2O will have 2.4088×10^24 hydrogen atoms.
8 0
3 years ago
When 1 mole of carbon is burned, carbon dioxide is produced, and 393 kilojoules (kJ) of energy are released. If this reaction is
EleoNora [17]
The energy of 393 kJ is released as heat.  Then, the container will experience an increase of temperature and, given that it is sealed, also an increase of pressure.

The increase of temperature results from the heat developed during the reaction.

The increase of pressure results from the fact that that the solid carbon will become gaseuos carbon dioxide. This gas will occupy a larger volume than the solid carbon and also this elevation of the temperature will make the pressure of the gas inside the container increase.

7 0
3 years ago
At 25 °C, how many dissociated OH– ions are there in 1243 mL of an aqueous solution whose pH is 2.07?
coldgirl [10]

<u>Answer:</u> The number of OH^- ions dissociated are 8.57\times 10^{11}

<u>Explanation:</u>

We are given:

pH = 2.07

Calculating the value of pOH by using equation, we get:

2.07+pOH=14\\\\pOH=14-2.07=11.93

To calculate hydroxide ion concentration, we use the equation to calculate pOH of the solution, which is:

pOH=-\log[OH^-]

We are given:

pOH = 11.93

Putting values in above equation, we get:

11.93=-\log[OH^-]

[OH^-]=10^{-11.93}=1.17\times 10^{-12}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 solution = 1.17\times 10^{-12}M

Volume of solution = 1243 mL = 1.243 L  (Conversion factor: 1 L = 1000 mL)

Putting values in above equation, we get:

1.17\times 10^{-12}M=\frac{\text{Moles of }OH^-}{1.243L}\\\\\text{Moles of }OH^-=(1.17\times 10^{-12}mol/L\times 1.243L)=1.424\times 10^{-12}mol

According to mole concept:

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

So, 1.424\times 10^{-12}mol number of OH^- will contain = (1.424\times 10^{-12}\times 6.022\times 10^{23})=8.57\times 10^{11} number of ions

Hence, the number of OH^- ions dissociated are 8.57\times 10^{11}

3 0
3 years ago
A supercomputer, nicknamed Roadrunner, built by IBM for the Los Alamos National Labs can perform about 1.03 petaflop/s (1 petafl
Dmitrij [34]

Answer:

18.5 years

Explanation:

(6 x 10^23)/(10^15 x 1.03 x 3600 x 24 x 365)

Hope this helps!

7 0
2 years ago
38. Identify the most important types of interparticle forces pres
zhannawk [14.2K]

Answer: im thinking its gonna be d.C2H6 and also

the explanation is on the research i had did before i had answered this question so i really hope this help :)

Explanation:

Ar = van de waals forces or london forces

C

H

4

= van de waals forces or london forces

HCl=permanent dipole-dipole interactions

CO = permanent dipole-dipole interactions

HF = hydrogen bonding

N

a

N

O

3

= permanent dipole-dipole interactions

C

a

C

l

2

= van de waals forces or london forces

4 0
3 years ago
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