Whats the correct answer ???

You are Investigating an organic compound. It has the following characteristics: an oxygen atom Is bonded to two carbon groups,

Vesna [10]

The correct answer most likely be c

7 0

4 years ago

What does molecule mean?

Bond [772]

A pure substance, only one type of atom

6 0

3 years ago

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How much energy is required to heat 87.1 g acetone (molar mass=58.08 g/mol) from a solid at -154.0°C to a liquid at -42.0°C? The

WARRIOR [948]

Answer:

The answer to the question above is

The energy required to heat 87.1 g acetone from a solid at -154.0°C to a liquid at -42.0°C = 29.36 kJ

Explanation:

The given variables are

ΔHfus = 7.27 kJ/mol

Cliq = 2.16 J/g°C

Cgas = 1.29 J/g°C

Csol = 1.65 J/g°C

Tmelting = -95.0°C.

Initial temperature = -154.0°C

Final temperature = -42.0°C?

Mass of acetone = 87.1 g

Molar mass of acetone = 58.08 g/mol

Solution

Heat required to raise the temperature of solid acetone from -154 °C to -95 °C or 59 °C is given by

H = mCsolT = 87.1 g* 1.65 J/g°C* 59 °C = 8479.185 J

Heat required to melt the acetone at -95 °C = ΔHfus*number of moles =

But number of moles = mass÷(molar mass) = 87.1÷58.08 = 1.5

Heat required to melt the acetone at -95 °C =1.5 moles*7.27 kJ/mol = 10.905 kJ

The heat required to raise the temperature to -42 degrees is

H = m*Cliq*T = 87.1 g* 2.16 J/g°C * 53 °C = 9971.21 J

Total heat = 9971.21 J + 10.905 kJ + 8479.185 J = 29355.393 J = 29.36 kJ

The energy required to heat 87.1 g acetone from a solid at -154.0°C to a liquid at -42.0°C is 29.36 kJ

4 0

3 years ago

Imagine that scientists have found a planet with an outer layer divided into plates made of hard, solid rock, but the mantle bel

VMariaS [17]

Answer:

well it could be mars

Explanation: it closer so its hotter but also there not almost the same

8 0

3 years ago

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Many computer chips are manufactured from silicon, which occurs in nature as SiO2 . When SiO2 is heated to melting, it reacts wi

Ierofanga [76]

Answer:

a. Theoretical yield of Si = 72.58 kg

b. Percent Yield = 91.2 %

Explanation:

The chemical reaction involved is: SiO₂ (l) + 2C (s) → Si (l) + 2CO (g)

The stoichiometric ratio = 1 mol SiO₂ ÷ 2 mol C = 0.5 mol SiO₂ ÷ 1 mol C

Given: mass of SiO₂: w₁ = 155.3kg = 155.3 × 10³g, mass of C: w₂ = 79.3kg = 79.3 × 10³g, mass of Si: w₃ = 66.2kg = 66.2 × 10³g (∵ 1 kg =1000g)

Molar mass of SiO₂: m₁ = 60.08 g/mol, atomic mass of C: m₂ = 12.01 g/mol, atomic mass of Si: m₃ = 28.08 g/mol

Number of moles of SiO₂ taken: n₁ = w₁ ÷ m₁ = 155300 g ÷ 60.08 g/mol = 2584.88 mol

Number of moles of C taken: n₂ = w₂ ÷ m₂ = 79300 g ÷ 12.01 g/mol = 6602.83 mol

Actual ratio = n₁ ÷ n₂ = 2584.88 mol SiO₂ ÷ 6602.83 mol C = 0.39 mol SiO₂ ÷ 1 mol C

Since the stoichiometric ratio > actual ratio

Therefore, SiO₂ is the limiting reagent.

Now, the mass of SiO₂ in 1 mol = number of moles × molar mass = 1 mol × 60.08 g/mol = 60.08 g

the mass of Si in 1 mol = number of moles × molar mass = 1 mol × 28.08 g/mol = 28.08 g

So 28.08 g of Si is produced from 60.08 g SiO₂

Therefore, the amount of Si produced from 155300 g SiO₂ = 155300 g × 28.08 g ÷ 60.08 g = 72583.62 g = 72.58 kg

Therefore, the theoretical yield of Si = 72.58 kg

Actual yield of Si = 66.2 kg

Therefore, Percent Yield = Actual yield ÷ Theoretical yield × 100 = 66.2 kg ÷ 72.58 kg × 100 = 91.2 %

3 0

3 years ago