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AleksAgata [21]
3 years ago
13

If 20 grams of N2 react completely with H2 , how many moles of NH3 are produced? Show Work

Chemistry
1 answer:
Maslowich3 years ago
5 0
This is the balanced eq
N2 + 3H2 -> 2NH3
first you need to find mole of N2 by using
mol = mass ÷ molar mass.
mol N2= 20g ÷ (14.01×2)g/mol
=0.7138mol
then look at the coefficient between H2 and NH3.
it is N2:NH3
1:2
0.7138:0.7138×2
0.7138:1.4276 moles
moles of NH3 = 1.4276 moles
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Answer:

attached below

Explanation:

Structure of two acyclic compounds with 3 or more carbons that exhibits one singlet in 1H-NMR spectrum

a) Acetone CH₃COCH₃

Attached below is the structure

b) But-2-yne (CH₃C)₂

Attached below is the structure

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3 years ago
Which is stronger - the attractive forces between water molecules and chromium and chloride ions, or the combined ionic bond str
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Answer is: the combined ionic bond strength of CrCl₂ and intermolecular forces between water molecules.

When chromium chloride (CrCl₂) is dissolved in water, the temperature of the water increases, heat of the solution is endothermic.

Dissociation of chromium chloride in water: CrCl₂(aq) → Cr²⁺(aq) + 2Cl⁻(aq).

Energy (the lattice energy) is required to pull apart the oppositely charged ions in chromium chloride.

The heat of hydration is liberated energy when the separated ions (in this example chromium cations and chlorine anions) attract polar water molecules.

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3 years ago
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You heat 51 grams of magnesium over a Bunsen burner for several minutes until it reacts with oxygen in the air. Then you weigh t
garik1379 [7]

Answer:

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Which side does the light always start from?
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2 years ago
A 0.245-L flask contains 0.467 mol co2 at 159 °c. Calculate the pressure using the ideal gas law.
lubasha [3.4K]

Answer:

Pressure, P = 67.57 atm

Explanation:

<u>Given the following data;</u>

  • Volume = 0.245 L
  • Number of moles = 0.467 moles
  • Temperature = 159°C
  • Ideal gas constant, R = 0.08206 L·atm/mol·K

<u>Conversion:</u>

We would convert the value of the temperature in Celsius to Kelvin.

T = 273 + °C

T = 273 + 159

T = 432 Kelvin

To find the pressure of the gas, we would use the ideal gas law;

PV = nRT

Where;

  • P is the pressure.
  • V is the volume.
  • n is the number of moles of substance.
  • R is the ideal gas constant.
  • T is the temperature.

Making P the subject of formula, we have;

P = \frac {nRT}{V}

Substituting into the formula, we have;

P = \frac {0.467*0.08206*432}{0.245}

P = \frac {16.5551}{0.245}

<em>Pressure, P = 67.57 atm</em>

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3 years ago
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