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2 years ago

10

What do climatologist study about fossil seashells in rock sediments to learn about climate

2 answers:

Arte-miy333 [17]2 years ago

7 0

Clues about the past climate are buried in sediments at the bottom of the oceans, locked away in coral reefs, frozen in glaciers and ice caps, and preserved in the rings of trees. Each of these natural recorders provides scientists with information about temperature, precipitation, and more.

ludmilkaskok [199]2 years ago

5 0

Answer:

What information can climatologists learn from fossils? Fossils of plants and animals can show adaptations that organisms had for a particular type of climate that existed millions of years ago. Climatologists look at many pieces of evidence to study climate change. These pieces of evidence can support each other.

Explanation:

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Silver sulfate dissociates into silver ions and sulfate ions:

bagirrra123 [75]

Answer:

A its a step by step equation the answer is A

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2 years ago

What do you call the things in an experiment that must be the same to make it fair

Pavel [41]

Answer:

controlled variables

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1 year ago

Read 2 more answers

For the following reaction, 4.31 grams of iron are mixed with excess oxygen gas . The reaction yields 5.17 grams of iron(II) oxi

natka813 [3]

<u>Answer:</u> The theoretical yield of iron (II) oxide is 5.53g and percent yield of the reaction is 93.49 %

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ ....(1)

<u>For Iron:</u>

Given mass of iron = 4.31 g

Molar mass of iron = 53.85 g/mol

Putting values in above equation, we get:

$\text{Moles of iron}=\frac{4.31g}{53.85g/mol}=0.0771mol$

For the given chemical reaction:

$2Fe(s)+O_2(g)\rightarrow 2FeO(s)$

By Stoichiometry of the reaction:

2 moles of iron produces 2 moles of iron (ii) oxide.

So, 0.0771 moles of iron will produce = $\frac{2}{2}\times 0.0771=0.0771mol$ of iron (ii) oxide

Now, calculating the theoretical yield of iron (ii) oxide using equation 1, we get:

Moles of of iron (II) oxide = 0.0771 moles

Molar mass of iron (II) oxide = 71.844 g/mol

Putting values in equation 1, we get:

$0.0771mol=\frac{\text{Theoretical yield of iron(ii) oxide}}{71.844g/mol}=5.53g$

To calculate the percentage yield of iron (ii) oxide, we use the equation:

$\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

Experimental yield of iron (ii) oxide = 5.17 g

Theoretical yield of iron (ii) oxide = 5.53 g

Putting values in above equation, we get:

$\%\text{ yield of iron (ii) oxide}=\frac{5.17g}{5.53g}\times 100\\\\\% \text{yield of iron (ii) oxide}=93.49\%$

Hence, the theoretical yield of iron (II) oxide is 5.53g and percent yield of the reaction is 93.49 %

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2 years ago

If a container contains 3.5 moles and has a volume of 1.5 L, then what volume is it when it contains 8 moles? *

Lilit [14]

Volume would be 3.4 L

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2 years ago

If we were to dissolve iodine in alcohol, which term would describe the alcohol?

marishachu [46]

It will be Solvent the term that would describe the alcohol will be solvent.

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2 years ago