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3 years ago

What is the only part of an atom that cannot change (either protons, neutrons, or electrons)?

1 answer:

3 0

The number of protons never changes in an atom. More electrons means a negative charge and fewer means a positive charge. Once an atom has an electrical charge it is called an ion. In an ion the atomic number and atomic mass do not change from the original.

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What is The relationship between a carnivore and an herbivore can be stated as

densk [106]

Predator and prey because herbivores are animals that only eat plants implying they wouldnt eat the carnivore as the carnivore would eat them because carnivores only eat animals such as the herbivore

not sure if that made sense but its B

3 0

2 years ago

What is the mass of 8.90 moles of magnesium chloride, MgCl2?

Korolek [52]

No of moles of MgCl2 = weight of MgCl2 / Molecular weight of MgCl2 Weight of MgCl2 =moles of MgCl2 x molecular mass of MgCl2 = 8.90 x 95=845.5 gm

6 0

3 years ago

What is the best description of the energy stored in a stretched or compressed object.

oksian1 [2.3K]

Answer:

Elastic Potential Energy

4 0

3 years ago

How many moles of coF3 are produced when 1.25 moles of 3co reacts

oee [108]

Answer:

1.25 moles

Explanation:

First, we need to balance the equation. Essentially, this means making sure we have the same number of each atom on each side.

On the left side, we currently have:

- 1 Co atom

- 2 F aomts

On the right side, we have:

- 1 Co atom

- 3 F atoms

To balance it, add a 2 to Co on the left, 3 to F2 on the left, and 2 to CoF3 on the right:

$2Co+3F_2$ → $2CoF_3$

Now, we have 1.25 moles of Co, and since the ratio between Co and CoF3 is 1:1, we also have 1.25 moles of CoF3.

Thus, the answer is 1.25 moles.

7 0

4 years ago

Read 2 more answers

A compound contains only carbon, hydrogen, and oxygen. combustion of 11.75 mg of the compound yields 17.61 mg co2 and 4.81 mg h2

Ymorist [56]

Number of moles is defined as the ratio of given mass in g to the molar mass.

First, convert the given mass of carbon dioxide in mg to g:

1 mg = 0.001 g

17.61 mg = 0.01761 g

Number of moles of carbon dioxide = $\frac{0.01761 g}{44.01 g/mol}$

= $0.0004001 mol$

Mass of carbon = number of moles of carbon dioxide \times molar mass of carbon

= $0.0004001 mol\times 12.011 g/mol$

= $0.004806 g$

Number of moles of water= $\frac{0.00481 g}{18 g/mol}$

= $2.672\times 10^{-4}$

Since, water contains two hydrogen atoms. Thus,

Moles of hydrogen = $2\times 2.672\times 10^{-4}$

= $5.34\times 10^{-4}$

Mass of hydrogen = $5.34\times 10^{-4}\times \times 1.008 g/mol$

= $5.34\times 10^{-4} g$

Mass of oxygen = $0.001175-(5.38\times 10^{-4}g+0.004806 g)$

= $0.006405 g$

Number of moles of oxygen = $\frac{0.006405 g}{15.999 g/mol}$

= $0.000400$

Now,

$C_{0.0004001} H_{0.000534} O_{0.000400}$

Divide the smallest number to get the whole number,

$C_{\frac{0.0004001}{0.000400}} H_{\frac{0.000534}{0.000400}} O_{\frac{0.000400}{0.000400}}$

we get,

$C_{1} H_{1.33} O_{1}$

Now, multiply all the subscript by 3 to get the whole number,

$C_{3} H_{4} O_{3}$ (empirical fomula)

Molar mass of the compound = $3\times 12.011 g/mol+4\times 1.008 g/mol+3\times 15.999 g/mol$

= $88.062 g/mol$

Divide given molar mass of the compound with the molar mass of the compound.

= $\frac{176.1 g/mol}{88.062 g/mol}$

= $1.999\simeq 2$

Thus, multiply the subscripts of empirical formula by 2 to get the molecular formula, we get:

$C_{6}H_{8}O_{6}$

Hence, empirical formula is $C_{3}H_{4}O_{3}$ and molecular formula is $C_{6}H_{8}O_{6}$

8 0

3 years ago