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mote1985 [20]
3 years ago
15

Which statement accurately describes the bond that forms between carbon and oxygen to create carbon dioxide

Chemistry
1 answer:
Allisa [31]3 years ago
8 0

Answer:

the bond that forms between carbon and oxygen to create carbon dioxide

A polar covalent bond

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(giving brainiest)<br><br> please answer correctly im failing school and these are my last points!
vesna_86 [32]

Answer:

i answered your other post with it

Explanation:

4 0
3 years ago
The block in this illustration is floating in water, which has a density of 1.00 g/cm3 .What is a good estimate of the density o
miss Akunina [59]

Answer : The density of the block is estimated to be, 0.30g/cm^3.

Explanation :

Density of the water, \rho_w=1.0 g/cm^3

As we know that,

Buoyant force = \rho\times volume\times g

where,

g = gravitational acceleration

volume of the block = v

density of the block = \rho_o

Weight of the Block = Buoyant force exerted by water

\rho_o\times v\times g=\rho_w\times 30\%\text{ of volume of block}\times g

\rho_o\times v\times g=\rho_w\times 0.30v\times g

\rho_o\times v\times 9.8 m/s^2=1 g/cm^3\times 0.30v\times 9.8 m/s^2

\rho_o=0.30 g/cm^3

Thus, the density of the block is estimated to be, 0.30g/cm^3.

6 0
3 years ago
In Part A, we saw that the theoretical yield of aluminum oxide is 0.700 mol . Calculate the percent yield if the actual yield of
s2008m [1.1K]

Considering the definition of percent yield, the percent yield is 76%.

<h3>Percent yield</h3>

The percent yield is the ratio of the actual return to the theoretical return expressed as a percentage.

The percent yield is calculated as the experimental yield divided by the theoretical yield multiplied by 100%:

percent yield=\frac{actual yield}{theorical yield}x100

where the theoretical yield is the amount of product acquired through the complete conversion of all reagents in the final product, that is, it is the maximum amount of product that could be formed from the given amounts of reagents.

<h3>Percent yield in this case</h3>

In this case, you know:

  • actual yield= 0.532 moles
  • theorical yield= 0.700 moles

Replacing in the definition of percent yield:

percent yield=\frac{0.532 moles}{0.700 moles}x100

Solving:

<u><em>percent yield= 76%</em></u>

Finally, the percent yield is 76%.

Learn more about percent yield:

brainly.com/question/14408642

#SPJ1

3 0
2 years ago
An atom has 9 electrons and 9 protons at the start. If it loses 2 electrons, the net charge on the atom will be . If the atom in
lara31 [8.8K]
Loses two = +2
gains 4 = -4
8 0
3 years ago
Read 2 more answers
First person with the right answer gets brainliest thanks (btw the numbers on the right are the answers choose the right one)
kap26 [50]
Molar mass of FE2O3=2(55.85)+3(16)=159.7

2.56g*1mol/159.7*2mol/1mol*55.85g/1mol=1.79g
6 0
3 years ago
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