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3 years ago

Which compound has the highest melting point? Al2(CO3)3 C12H22O11 C8H18 H2O

Chemistry

2 answers:

Rasek [7]3 years ago

6 0

Answer:

Al2(CO3)3 (A)

Explanation:

i think thats the answer

klasskru [66]3 years ago

3 0

Answer:

Explanation:

Al2(CO3)3 has a melting point of 58 celcius

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Intermolecular forces allow which of the following substances to be the least fluid?

slava [35]

Out of the options, glass is the least fluid. The proof of this also lies in the fact that glass is the most difficult to melt out of all of the mentioned substances, and melting point gives us a rough estimate of the strength of intermolecular forces.

3 0

4 years ago

Read 2 more answers

A rope has one end tied to a vertical support. You hold the other end so that the rope is horizontal. If you move the end of the

Lady_Fox [76]

Answer:

The speed of the wave in the rope is 2 m/s

Explanation:

1. Data:

a) ν = 4 Hz

b) λ = 0.5 m

c) s = ?

2. Physical principles and formula:

The propagation of waves in a rope is a classical example of transverse waves: the pulse is inflected in the vertical direction and the wave travels in the horizontal direction, i.e. the pulse or vibration is perpendicular to the motion of the media particles.

The equation that relates speed (s), wavelength (λ), frequency (ν) is:

distance = speed × time

wavelength = speed × period

wavelenfth = speed / frequency

λ = s / ν

meter = (meter/second) / second⁻¹

m = (m /s) / s⁻¹

3. Solution:

λ = s / ν⇒ s = λ·ν

s = 0.5 m × 4 Hz = 2 m/s

5 0

3 years ago

In a blast furnace, iron(III) oxide is used to produce iron by the following (unbalanced) reaction: Fe2O3 + CO---------->Fe +

rewona [7]

Answer:

a) The no. of moles of CO are needed = 75.15 mol.

b) The no. of moles of Fe are produced = 50.1 mol.

The no. of moles of CO₂ are needed = 75.15 mol.

Explanation:

Firstly, we need to write the balanced reaction:

Fe₂O₃ + 3CO → 2Fe + 3CO₂,

It is clear that 1 mol of Fe₂O₃ reacts with 3 mol of CO to produce 2 mol of Fe and 3 mol of CO₂.

a) If 4.00 kg Fe₂O₃ are available to react, how many moles of CO are needed?

We need to calculate the no. of moles of 4.00 kg Fe₂O₃:

n = mass/molar mass = (4000 g)/(159.69 g/mol) = 25.05 mol.

Using cross multiplication:

1 mol of Fe₂O₃ need → 3 mol of CO to react completely, from stichiometry.

25.05 mol of Fe₂O₃ need → ??? mol of CO to react completely.

∴ The no. of moles of CO are needed = (3 mol)(25.05 mol)/(1 mol) = 75.15 mol.

b) How many moles of each product are formed?

To find the no. of moles of Fe formed:

Using cross multiplication:

1 mol of Fe₂O₃ produce → 2 mol of Fe, from stichiometry.

25.05 mol of Fe₂O₃ produce → ??? mol of Fe.

∴ The no. of moles of Fe are produced = (2 mol)(25.05 mol)/(1 mol) = 50.1 mol.

To find the no. of moles of CO₂ formed:

Using cross multiplication:

1 mol of Fe₂O₃ produce → 3 mol of CO₂, from stichiometry.

25.05 mol of Fe₂O₃ produce → ??? mol of CO₂.

∴ The no. of moles of CO₂ are needed = (3 mol)(25.05 mol)/(1 mol) = 75.15 mol.

4 0

3 years ago

consider the reaction below. CO(g)=Cl2(g)=COCl2(g). what is the most likely effect to the forward reaction if there is an increa

tiny-mole [99]

B) The reaction rate decreases

4 0

4 years ago

Convert 6.35 grams of aluminum sulfate to moles

vampirchik [111]

Answer:

There are 0.0186 moles of formula units in 6.35 grams of aluminum sulfate $\rm Al_2(SO_4)_3$ .

Explanation:

What's the empirical formula of aluminum sulfate?

Sulfate is an anion with a charge of -2 per ion. When sulfate ions are bonded to metals, the compound is likely ionic.

Aluminum is a group III metal. Its ions tend to carry a charge of +3 per ion.

The empirical formula of an ionic compound shall balance the charge on ions with as few ions as possible.

The least common multiple of 2 and 3 is 6. That is:

Three sulfate ions $\rm {SO_4}^{2-}$ will give a charge of -6.
Two aluminum ions $\rm Al^{3+}$ will give a charge of +6.

Pairing three $\rm {SO_4}^{2-}$ ions with two $\rm Al^{3+}$ will balance the charge. Hence the empirical formula: $\rm Al_2(SO_4)_3$ .

What's the mass of one mole of aluminum sulfate? In other words, what's the formula mass of $\rm Al_2(SO_4)_3$ ?

Refer to a modern periodic table for relative atomic mass data:

Al: 26.982;
S: 32.06;
O: 15.999.

There are

two Al,
three S, and
twelve O

in one formula unit of $\rm Al_2(SO_4)_3$ .

Hence the formula mass of $\rm Al_2(SO_4)_3$ :

$\underbrace{2\times 26.982}_{\rm Al} + \underbrace{3\times 32.06}_{\rm S} + \underbrace{12\times 15.999}_{\rm O} = \rm 342.132\;g\cdot mol^{-1}$ .

How many moles of formula units in 6.35 grams of $\rm Al_2(SO_4)_3$ ?

$\displaystyle n = \frac{m}{M} = \rm \frac{6.35\;g}{342.132\;g\cdot mol^{-1}} = 0.0186\;mol$ .

8 0

3 years ago