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arsen [322]
2 years ago
8

The ratio of carbon-14 to carbon-12 in a piece of charcoal from a fire pit in an archaeological excavation is found to be 12.5%

of that in a sample of modern wood. Approximately how old is the site? (Carbon-14 half-life is 5730 years.) Answer as a whole number with no units.
Chemistry
1 answer:
blagie [28]2 years ago
3 0

Answer:

17190 years          

Explanation:

The exponential decay equation is:

N_{t} = N_{0}e^{-\lambda t}          

\frac{N_{t}}{N_{0}} = e^{-\lambda t}

Where:

N(t) is the quantity at time t

N₀ is the initial amount

λ is the decay constant = ln(2)/t(1/2)

t(1/2) is the half-life    

Since the ratio of carbon-14 to carbon-12 is 12.5%, we have that:

\frac{N_{t}}{N_{0}} = e^{-\lambda t}

\frac{0.125N_{0}}{N_{0}} = e^{-\lambda t}

ln(0.125) = -\lambda t

By solving the above equation for t:

t = \frac{ln(0.125)}{-\lambda} = \frac{ln(0.125)}{-ln(2)/t_{1/2}} = \frac{5730 y* ln(0.125)}{-ln(2)} = 17190 y

                                               

Therefore, the site is 17190 years old.  

                                                                       

I hope it helps you!

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17. What is the molarity of ZnCl2 that forms when 15 grams of Zn reacts completely with CuCl, if a
GalinKa [24]

Answer:

1.31M

Explanation:

Based on the reaction, 1 mole of Zn produce 1 mole of ZnCl₂. As the reaction occurs completely, the moles of Zn added = Moles of ZnCl₂ produced. To find molarity we need the moles of ZnCl₂ and the volume of the solution in liters:

<em>Moles Zn = Moles ZnCl₂ -Molar mass Zn: 65.38g/mol-:</em>

15g * (1mol / 65.38g) = 0.23 moles of ZnCl₂

<em>Volume in Liters:</em>

175mL * (1L / 1000mL) = 0.175L

The molarity is:

0.23moles / 0.175L

<h3>1.31M</h3>
7 0
2 years ago
Can someone explain me why the molar mass become 90.12 g/mol and when I calculated it's 90 g/mol?​
e-lub [12.9K]

Answer:

It could be because of rounding error somewhere in your calculations. Another thing to note is 90 +/- 4 g/mol.

Your calculations don't have to be spot on.

8 0
3 years ago
A chemist dilutes a 1.0 ml sample of 2.0 m kno3 by adding water to it. if the concentration of the solution that is obtained is
Nitella [24]

A chemist dilutes a 1.0 ml sample of 2.0M KNO₃ by adding water to it. If the concentration of the solution that is obtained is 0.0080 m, then its volume is 250mL.

<h3>How do we calculate volume?</h3>

Volume for the given equation will be calculated by using the below equation as:

M₁V₁ = M₂V₂, where

M₁ = molarity of KNO₃ = 2M

V₁ = volume of KNO₃ = 1mL

M₂ = molarity of final solution = 0.0080M

V₂ = volume of final solution = ?

On putting these values on the above equation, we get

V₂ = (2)(1) / (0.0080) = 250mL

Hence option (2) is correct.

To know more about molarity, visit the below link:

brainly.com/question/24305514

8 0
2 years ago
How many moles of oxygen gas occupy 67.2 L of volume at STP?<br> A 0.333<br> B 3.00<br> C 1.00
posledela

Answer:

I would say b hope this helps

Explanation:

have a good day btw i had this question before:D

7 0
3 years ago
One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silv
babunello [35]

Answer:

5.0x10⁻⁵ M

Explanation:

It seems the question is incomplete, however this is the data that has been found in a web search:

" One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose a EPA chemist tests a 250 mL sample of groundwater known to be contaminated with nickel(II) chloride, which would react with silver nitrate solution like this:

NiCl₂ + 2AgNO₃ →  2AgCl + Ni(NO₃)₂

The chemist adds 50 mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 3.6 mg of silver chloride. Calculate the concentration of nickel(II) chloride contaminant in the original groundwater sample. Round your answer to 2 significant digits. "

Keep in mind that while the process is the same, if the values in your question are different, then your answer will be different as well.

First we <u>calculate the moles of nickel chloride found in the 250 mL sample</u>:

  • 3.6 mg AgCl ÷ 143.32 mg/mmol * \frac{1mmolNiCl_{2}}{2mmolAgCl} = 0.0126 mmol NiCl₂

Now we <u>divide the moles by the volume to calculate the molarity</u>:

  • 0.0126 mmol / 250 mL = 5.0x10⁻⁵M
4 0
3 years ago
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