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4 years ago

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Chemists recognize many different elements, such as gold, or oxygen, or carbon, or iron. suppose you got some iron, and started

splitting it into smaller pieces. the smallest piece that would still be called 'iron' would be:

1 answer:

Leni [432]4 years ago

5 0

The answer is atom i hope it helps

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The atomic mass of beryllium (Be) is 9.01 amu. The atomic mass of calcium (Ca), which is in the same group as beryllium, is 40.0

bekas [8.4K]

Mg will have a higher amu than Be but a lower amu than Ca.

8 0

3 years ago

Read 2 more answers

A 2 kg toy car and a 5 kg toy car are pushed with an equal amount of force. Which toy car will have the least acceleration?

pishuonlain [190]

Answer:

The 5 kg toy car will have least acceleration

Explanation:

3 0

3 years ago

If 1.332 mol of C4H10 are reacted with 6.504 mol of O2, how many mol of the excess reagent will remain unreacted? 2 C4H10 + 13 O

Luden [163]

Answer: The number of moles of excess reagent remain unreacted will be, 6.004 moles.

Explanation : Given,

Moles of $C_4H_{10}$ = 1.332 mol

Mass of $O_2$ = 6.504 mol

First we have to calculate the limiting and excess reagent.

The balanced chemical equation is:

$C_4H_{10}+13O_2\rightarrow 10H_2O+8CO_2$

From the balanced reaction we conclude that

As, 13 mole of $O_2$ react with 1 mole of $C_4H_{10}$

So, 6.504 moles of $O_2$ react with $\frac{6.504}{13}=0.5003$ moles of $C_4H_{10}$

From this we conclude that, $C_4H_{10}$ is an excess reagent because the given moles are greater than the required moles and $O_2$ is a limiting reagent and it limits the formation of product.

Number of moles remain unreacted = 6.504 mol - 0.5003 mol = 6.004 mol

Therefore, the number of moles of excess reagent remain unreacted will be, 6.004 moles.

5 0

4 years ago

The decomposition of N2O to N2 and O2 is a first-order reaction. At 730°C, the rate constant of the reaction is 1.94 × 10-4 min-

lara31 [8.8K]

Answer:

the total gas pressure after one half-life is 4.38 atm

Explanation:

The balanced equation for the decomposition of N2O to N2 and O2 is given as:

2N₂O(gas) ⇒ 2N₂(gas) + O₂(gas)

2 moles of N₂O produce 2 moles of N₂ and 1 mole of O₂

The change in pressure depends on the coefficient (number of moles) of the reactant and product.

N₂O N₂ O₂

number of moles 2 2 1

Initial pressure (atm) 3.50 0 0

change in pressure -2x +2x x

Final pressure (atm) 3.50 - 2x 2x x

The total final pressure is the sum of the individual total pressure. i.e.:

Total final pressure = final pressure of N₂O + final pressure of N₂ + final pressure of O₂

Total final pressure = (3.5 - 2x) + (2x) + x

Total final pressure = 3.5 + x

After one half life, the initial pressure of N₂O would be half its value.

Final pressure of N₂O = half of the initial pressure of N₂O

3.5 - 2x = 0.5(3.5)

3.5 - 2x = 1.75

2x = 1.75

x = 0.875 atm

Therefore, Total final pressure = 3.5 + x = 3.5 + 0.875

Total final pressure = 4.38 atm to 3 significant figures

4 0

3 years ago

How is precipitation useful in our daily lives?

Alex73 [517]

Answer:

The precipitation reaction is the double displacement reaction in which two ionic bonds combine forming up insoluble salts.

Precipitation reaction can be used in our daily life in events such as in waste water treatment. When a contaminant forms an insoluble solid, then we can use this reaction to precipitate out the contaminated ions.

The rings which form in the bathtubs are also an example of the precipitation reactions.

3 0

4 years ago