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3 years ago

A/1 * B/C = D

Chemistry

1 answer:

Anit [1.1K]3 years ago

3 0

Answer: 0.64 Moles of Propane

Explanation:

Data:

Moles of Carbon = 1.5 mol

Conversion factor = 7 mol C produces = 3 mol of Propane

Solution:

As we know,

7 moles of Carbon produces = 3 moles of Propane

Then,

1.5 moles of Carbon will produce = X moles of Propane

Solving for X,

X = (1.5 moles × 3 moles) ÷ 7 moles

X = 0.6428571 moles of Propane

Or rounded to two significant figures,

X = 0.64 Moles of Propane

Read more on Brainly.com - brainly.com/question/11464115#readmore

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Korvikt [17]

Answer:

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3 years ago

What are the TWO characteristics of an effective collision?

Montano1993 [528]

Answer:

the TWO characteristics of an effective collision are:

1.Molecules collide with sufficient energy

2.Molecules collide with the proper orientation.

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3 years ago

21. In infrared spectroscopy, absorption of electromagnetic radiation results in transitions between ________ energy levels.

Slav-nsk [51]

In infrared spectroscopy, absorption of electromagnetic radiation results in transitions between <u>Vibrational </u>energy levels.

<h3>What does spectroscopy mean?</h3>

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5 0

2 years ago

Trichloroethylene, a widely used degreasing solvent for machine parts, is produced in a two-step reaction sequence. Ethylene is

solmaris [256]

Answer:

ΔH°C2H2Cl4(l) = -333,36 kJ/mol

ΔH°r₂ = -35,14 kJ/mol

Explanation:

The ΔH°r of the first reaction is:

ΔH°r = -385,76 kJ/mol = (ΔH°C2H2Cl4(l) + ΔH°H2(g)) - (ΔH°C2H4(g) + 2ΔHCl2 (g))

ΔH°H2(g) = 0 kJ/mol

ΔH°C2H4(g) = 52,4 kJ/mol

Δ°HCl2 (g) = 0 kJ/mol

Replacing:

ΔH°C2H2Cl4(l) = -385,76 kJ/mol + 52,4 kJ/mol = <em>-333,36 kJ/mol</em>

The standard heat of the second reaction is:

ΔH°r₂ = ΔH°C2HCl3(l) + ΔH°HCl(g) - ΔH°C2H2Cl4(l)

Where:

ΔH°C2HCl3(l) = -276,2 kJ/mol; ΔH°HCl(g) = -92,3 kJ/mol; ΔH°C2H2Cl4(l) = -333,36 kJ/mol

Replacing:

ΔH°r₂ = -276,2 kJ/mol -92,3 kJ/mol + 333,36 kJ/mol

I hope it helps!

4 0

3 years ago

Can someone check my work?

sesenic [268]

it seems right good work

7 0

3 years ago