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Vikentia [17]
2 years ago
10

How many grams are there in 9.03 x 1023 molecules of CO2?

Chemistry
1 answer:
wariber [46]2 years ago
5 0

Answer:

The correct answer is - 66g.

Explanation:

Given:

molecules of CO2 = 9.03 x 10^23

We know:

1 mole of any substance = 6.02x10^23 molecules. (Avogadro's number)

M (CO2) = 12 + (2x16) = 12 + 32 = 44g

Solution:

The mass of CO2 with 9.03x10^23 molecules would be:

44g of CO2 = 6.02x10^23 molecules.

So, the mass in grams of CO2 (X) = 9.03x10^23 molecules

Xg of CO2 = (44x9.03x10^23)/6.02x10^23 = 66g

Thus, the correct answer would be - 66gm.

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H+ ions are proton charged ions that are present
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According to the cooling curve, what is the approximate freezing point of the substance?
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Correct answer: B

Cooling curve is the plot of temperature versus time as the sample is allowed to cool. In a cooling curve, we start at a temperature greater than the boiling point. At this temperature, the sample is in gaseous state. At the boiling point, there is no change in temperature as the gaseous and liquid states are in equilibrium. As the temperature reduces further, the liquid starts to condense and at the melting point of the sample the liquid undergoes phase transition to solid state. At the melting temperature, a second plateau is observed as the temperature remains unchanged. At temperatures below the melting point, the sample exists as a solid.

So from the curve, the second plateau is observed at around -111^{0}C. This point represents the phase transition from liquid to solid state.

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2Al + 3H2SO4 -> Al2(SO4)3 + 3H2How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with alumi
bazaltina [42]

Answer:

290.82g

Explanation:

The equation for the reaction is given below:

2Al + 3H2SO4 -> Al2(SO4)3 + 3H2 now, let us obtain the masses of H2SO4 and Al2(SO4)3 from the balanced equation. This is illustrated below:

Molar Mass of H2SO4 = (2x1) + 32 + (16x4) = 2 + 32 +64 = 98g/mol

Mass of H2SO4 from the balanced equation = 3 x 98 = 294g

Molar Mass of Al2(SO4)3 = (2x27) + 3[32 + (16x4)]

= 54 + 3[32 + 64]

= 54 + 3[96] = 54 + 288 = 342g

Now, we can obtain the mass of aluminium sulphate formed by doing the following:

From the equation above:

294g of H2SO4 produced 342g of Al2(SO4)3.

Therefore, 250g of H2SO4 will produce = (250 x 342)/294 = 290.82g of Al(SO4)3

Therefore, 290.82g of aluminium sulphate (Al(SO4)3) is formed.

7 0
3 years ago
Which of these statements describes a physical property of hydrogen? Group of answer choices it is found in acids. it is less de
pochemuha

Answer:

it is less dense than oxygen gas.

Explanation:

Hydrogen is the simplest chemical element that exists. The symbol for the chemical element Hydrogen is "H" and it is a colourless, tasteless, odorless, and highly flammable gas.

Hydrogen is a chemical element found in group (1) of the periodic table and as such it has one (1) electrons in its outermost shell. Therefore, Hydrogen has an atomic number of one (1) and a single valence electrons because it has only one proton and one electron in its nucleus.

In Chemistry, the properties of a chemical element that can be observed and measured without changing its chemical nature is known as a physical property. It includes density, color, freezing point, opacity, smell, melting point, viscosity, etc.

Hence, the statement which describes a physical property of hydrogen is that it is less dense (density) than oxygen gas.

7 0
2 years ago
a 1.25g sample of ore containing iron pyrite (FeS2) was pulverized and ignited in air, converting the FeS2 to Fe2O3 and SO2(g).
svp [43]

Answer:

28.9%

Explanation:

Let's consider the following balanced equation.

2 FeS₂ + 11/2 O₂ ⇒ Fe₂O₃ + 4 SO₂

We can establish the following relations:

  • The molar mass of Fe₂O₃ is 159.6 g/mol
  • 1 mole of Fe₂O₃ is produced per 2 moles of FeS₂
  • 1 mole of Fe is in 1 mole of FeS₂
  • The molar mass of Fe is 55.84 g/mol

The amount of Fe in the sample that produced 0.516 g of Fe₂O₃ is:

0.516gFe_{2}O_{3}.\frac{1molFe_{2}O_{3}}{159.6gFe_{2}O_{3}} .\frac{2molFeS_{2}}{1molFe_{2}O_{3}} .\frac{1molFe}{1molFeS_{2}} .\frac{55.84gFe}{1molFe} =0.361gFe

The percent of Fe in 1.25 g of the ore is:

\frac{0.361g}{1.25g} .100\%=28.9\%

4 0
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