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3 years ago

13

An example of a double replacement chemical reaction takes place in batteries. In an alkaline battery, Manganese oxide reacts wi

th water to form a different manganese oxide and hydroxide. Which is the correct balanced equation for this?

1 answer:

ozzi3 years ago

6 0

Answer:

2MnO2 + H2O => Mn2O3 + 2OH is the correct balanced equation.

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I am a celestial body that does not produce light. I orbit a planet

Artyom0805 [142]

A moon would be the correct answer.

5 0

3 years ago

A solution has a hydrogen ion concentration of 6.8 10–3 M. (2 points) i. What is the pH of the solution? Show your work.

vladimir2022 [97]

Answer:

2.17

Explanation:

To calculate pH using the hygrogen ion concentration we must use the following formula:

- log (H+) = pH

All we have to do now is plug in our hygrogen ion concentration and put it in our calculator.

- log (6.8 × 10⁻³) = 2.17

Don't forget proper figures for pH!

8 0

3 years ago

Sodium is an inactive metal why

Sphinxa [80]

Answer:

Inactive metals are inert metals that doesn’t react with most of the chemicals.They are highly resistant to oxidation and corrosion when exposed to moisture.

Explanation:

7 0

3 years ago

The mass percent of carbon in a typical human is 18%, and the mass percent of 14C in natural carbon is 1.6 × 10-10%. Assuming a

Tema [17]

Answer:

4066 decay/s

Explanation:

Given that:-

The weight of the person is:- 190 lb

Also, 1 lb = 453.592 g

So, weight of the person = 86182.6 g

Also, given that carbon is 18% in the human body. So,

$\%\ Carbon=\frac{18}{100}\times 86182.6\ g=15512.868\ g$

Carbon-14 is $1.6\times 10^{-10}\ \%$ of the carbon in the body. So,

$\%\ Carbon-14=\frac{1.6\times 10^{-10}}{100}\times 15512.868\ g=2.48\times 10^{-8}\ g$

Also,

14 g of Carbon-14 contains $6.023\times 10^{23}$ atoms of carbon-14

So,

$2.48\times 10^{-8}\ g$ of Carbon-14 contains $\frac{6.023\times 10^{23}}{14}\times 2.48\times 10^{-8}$ atoms of carbon-14

Atoms of carbon-14 = $1.07\times 10^{15}$

Given that:

Half life = 5730 years

$t_{1/2}=\frac {ln\ 2}{k}$

Where, k is rate constant

So,

$k=\frac {ln\ 2}{t_{1/2}}$

$k=\frac{ln\ 2}{5730}\ years^{-1}$

The rate constant, k = 0.00012 years⁻¹

Also, 1 year = $3.154\times 10^7$ s

So, The rate constant, k = $\frac{0.00012}{3.154\times 10^7}$ s⁻¹ = $3.8\times 10^{-12}\ s^{-1}$

Thus, decay events per second = $K\times atoms decayed$ = $3.8\times 10^{-12}\times 1.07\times 10^{15}\ decay/s$ = 4066 decay/s

4 0

3 years ago

How many atoms are present in 0.35 mol of carbon dioxide?

STatiana [176]

0.35 moles carbon dioxide (6.022 X 10^23/1 mole CO2) = 2.1 X 10^23 atoms of
<span> carbon dioxide </span>

6 0

3 years ago

Read 2 more answers