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3 years ago

Octane has a higher boiling point than pentane because _____.

1 answer:

6 0

Octane has a higher boiling point than pentane because it contains a higher amount of atoms specifically carbon than the number of propane found on it. You can find a large number of London dispersion which is attractive forces than butane.

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How much does the earth weigh?

Lady_Fox [76]

Answer:

5.972 × 10^24 kg

3 0

3 years ago

N2(g) + 3H2(g) →2NH3(g)

monitta

Answer:

2.5 moles of N₂ and 7.5 moles of H₂ entered the reaction

Explanation:

In reaction:

N₂(g) + 3 H₂(g) → 2 NH₃(g)

You can see that the stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction) requires the following amounts of reagents and are produced:

N₂: 1 mole
H₂: 3 moles
NH₃: 2 moles

The following three rules can apply:

If 2 moles of NH₃ are produced from 1 mole of N₂ by stoichiometry of the reaction, 5 moles of NH₃ from how many moles of N₂ are produced?

$moles of N_{2} =\frac{5 moles of NH_{3} *1 mole of N_{2} }{2 moles of NH_{3}}$

moles of N₂= 2.5

If 2 moles of NH₃ are produced from 3 moles of H₂ by stoichiometry of the reaction, 5 moles of NH₃ from how many moles of H₂ are produced?

$moles of H_{2} =\frac{5 moles of NH_{3} *3 mole of H_{2} }{2 moles of NH_{3}}$

moles of H₂= 7.5

2.5 moles of N₂ and 7.5 moles of H₂ entered the reaction

6 0

3 years ago

At STP, which gas sample has a volume of 11.2 liters?

Natasha2012 [34]

Answer:

0.500 moles of CO2 has a volume of 11.2 L at STP (option B)

Explanation:

Step 1: Data given

Volume of a gas at STP = 11.2 L

STP: Pressure = 1 atm and temperature = 273 K

Step 2: Calculate volume

p*V= n*R*T

V = (n*R*T)/p

⇒with V = the volume of the gas = TO BE DETERMINED

⇒with n = the number of moles of the gas

⇒with R = the gas constant = 0.08206 L*atm/mol*K

⇒with T = the temperature = 273 K

⇒with p = the pressure of the gas = 1 atm

A ) 0.250 mole of NH3

V = (0.250 * 0.08206 * 273) / 1

V = 5.6 L

B ) 0.500 mole of CO2

V = (0.500 * 0.08206 * 273) / 1

V = 11.2 L

C ) 0.750 mole of NH3

V = (0.750 * 0.08206 * 273) / 1

V = 16.8 L

D) 1.00 mole of CO2

V = (1.00 * 0.08206* 273) / 1

V = 22.4 L

0.500 moles of CO2 has a volume of 11.2 L at STP (option B)

3 0

4 years ago

What is the volume, in liters, of 2.00 moles of hydrogen at STP?

Ber [7]

The volume of one mole of any gas at STP is 22.4 L. So, at STP, the volume of 2.00 moles of hydrogen gas would be (22.4 L/mol)(2 mol H2) = 44.8 L.

8 0

3 years ago

Which of the following is an expression of Charles's law?

HACTEHA [7]

Answer:

Explanation:

V/T

4 0

3 years ago