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3 years ago

Can atoms combine in different ways to make up all of the substances you encouter every day

1 answer:

8 0

Majority can such as hydrogen H and oxygen O forming water H2O but uranium having extra neutrons to form plutonium and beyond simply can't because it will not last for a fraction of a second or spiral out of control and violently react like the little boy and the fat man (a uranium and plutonium nuclear weapon) so yes and no

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When a parent has alleles for a dominant trait, what traits show up in the offspring?

Effectus [21]

Try putting this in biology category not chemistry so more ppl can help :)

4 0

3 years ago

A sample of mass 6.814 grams is added to another sample weighing 0.08753 grams.

Feliz [49]

Answer:

17.5609g

Explanation:

According to the question, a sample of mass 6.814 grams is added to another sample weighing 0.08753 grams. That is weight of sample 1 + weight of sample 2;

6.814 + 0.08753 = 6.90153grams

Next, the subsequent mixture is then divided into exactly 3 equal parts i.e. 6.90153grams divided by 3

= 6.90153/3

= 2.30051grams.

One of the equal parts is 2.30051grams, which is then multiplied by 7.6335 times I.e. 2.30051 × 7.6335 = 17.5609grams

Therefore, the final mass is 17.5609grams

3 0

3 years ago

What is the valence shell electronic configuration of Alkali Metals , Alkaline Earth Metals, Halogens and Noble Gases?

alisha [4.7K]

Answer:

alkali metals: 1

alkaline earth metals: 2

Halogens: 7

noble gases : 8

3 0

2 years ago

Read 2 more answers

Iron (III) oxide and hydrogen react to form iron and water, like this: Fe 03(s)+3H9)2Fe(s)+3HO) At a certain temperature, a chem

belka [17]

The question is incomplete, here is the complete question:

Iron (III) oxide and hydrogen react to form iron and water, like this:

$Fe_2O_3(s)+3H_2(g)\rightarrow 2Fe(s)+3H_2O(g)$

At a certain temperature, a chemist finds that a 8.9 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, Iron, and water at equilibrium has the following composition.

Compound Amount

Fe₂O₃ 3.95 g

H₂ 4.77 g

Fe 4.38 g

H₂O 2.00 g

Calculate the value of the equilibrium constant Kc for this reaction. Round your answer to 2 significant digits.

Answer: The value of equilibrium constant for given equation is $1.0\times 10^{-4}$

Explanation:

To calculate the molarity of solution, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Mass of solute}}{\text{Molar mass of solute}\times \text{Volume of solution (in L)}}$

For hydrogen gas:

Given mass of hydrogen gas = 4.77 g

Molar mass of hydrogen gas = 2 g/mol

Volume of the solution = 8.9 L

Putting values in above expression, we get:

$\text{Molarity of hydrogen gas}=\frac{4.77}{2\times 8.9}\\\\\text{Molarity of hydrogen gas}=0.268M$

For water:

Given mass of water = 2.00 g

Molar mass of water = 18 g/mol

Volume of the solution = 8.9 L

Putting values in above expression, we get:

$\text{Molarity of water}=\frac{2.00}{18\times 8.9}\\\\\text{Molarity of water}=0.0125M$

For the given chemical equation:

$Fe_2O_3(s)+3H_2(g)\rightarrow 2Fe(s)+3H_2O(g)$

The expression of equilibrium constant for above equation follows:

$K_{eq}=\frac{[H_2O]^3}{[H_2]^3}$

Concentration of pure solids and pure liquids are taken as 1 in equilibrium constant expression.

Putting values in above expression, we get:

$K_{c}=\frac{(0.0125)^3}{(0.268)^3}\\\\K_{c}=1.0\times 10^{-4}$

Hence, the value of equilibrium constant for given equation is $1.0\times 10^{-4}$

6 0

3 years ago

On the space shuttle, lithium hydroxide is produced from lithium oxide and water. The lithium hydroxide then reacts with the exh

Ratling [72]

Answer:

6,2g of CO₂

Explanation:

Based on the reactions:

Li₂O(s) + H₂O(g) → 2LiOH(s)

LiOH(s) + CO₂(g) → LiHCO₃(s)

2,6g of Li₂O and 1,3g of H₂O are:

2,6g × ( 1mol / 29,88g) = 0,087 moles

1.3g × ( 1mol / 18,01g) = 0,072 moles

That means limiting reactant is H₂O. The moles produced of LiOH are:

0,072 moles of H₂O × ( 2mol LiOH / 1mol H₂O) = 0,14 moles of LiOH

Thus, the maximum CO₂ that can react are 0,14 moles of CO₂, in grams

0,14 moles CO₂ × (44,01g / 1mol) = 6,2g of CO₂

I hope it helps!

6 0

2 years ago