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aliina [53]
3 years ago
14

Write the net ionic equation for the reaction of sodium chloride with magnesium hydroxide. Include the complete ionic equation a

nd label spectator ions. Also be sure to label the reactants and products as solid, liquid, gas, or aqueous solutions.
Chemistry
2 answers:
Lera25 [3.4K]3 years ago
8 0
Idk idk idk idk Idk idk idk idk idk Idk idk idk idk idk Idk idk idk idk idk
svp [43]3 years ago
7 0
This a long process...
first you write down the equation,in this case:
2NaCl (aq) + Mg(OH)2 (s) ———> MgCl2 (aq) + 2NaOH (aq) .
next you break them up into ions :
(only break up the aqueous solutions)
(2Na+) + (2Cl-) + Mg(OH)2 {leave it together} ———> (Mg2+) + (2Cl-) + (2Na+) + (2OH-).
then look at both sides of equation and cancel the ions that appear twice .
In this case: Cl and Na.
now the remaining is your final net atomic equation:
Mg(OH)2———-> Mg2 + 2OH.
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Inertia  decelerates a body.
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Help please, 44 to 45, calculate the answers to the following problems. Use the following equation as the basis of your calculat
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Answer: 44,8 l. of CO2 and 72 g. of water will be produced

Explanation:

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A mixture containing nitrogen and hydrogen weighs 3.49 g and occupies a volume of 7.45 L at 305 K and 1.03 atm. Calculate the ma
-BARSIC- [3]

Answer:

Mass percent N₂ = 89%

Mass percent H₂ = 11%

Explanation:

First we <u>use PV=nRT to calculate n</u>, which is the total number of moles of nitrogen and hydrogen:

  • 1.03 atm * 7.45 L = n * 0.082 atm·L·mol⁻¹·K⁻¹ * 305 K
  • n = 0.307 mol

So now we know that

  • MolH₂ + MolN₂ = 0.307 mol

and

  • MolH₂ * 2 g/mol + MolN₂ * 28 g/mol = 3.49 g

So we have a <u>system of two equations and two unknowns</u>. We use algebra to solve it:

Express MolH₂ in terms of MolN₂:

  • MolH₂ + MolN₂ = 0.307 mol
  • MolH₂ = 0.307 - MolN₂

Replace that value in the second equation:

  • MolH₂ * 2 g/mol + MolN₂ * 28 g/mol = 3.49
  • (0.307-MolN₂) * 2 + MolN₂ * 28 = 3.49
  • 0.614 - 2MolN₂ + 28molN₂ = 3.49
  • 0.614 + 26MolN₂ = 3.49
  • MolN₂ = 0.111 mol

Now we calculate MolH₂:

  • MolH₂ + MolN₂ = 0.307 mol
  • MolH₂ + 0.111 = 0.307
  • MolH₂ = 0.196 mol

Finally, we convert each of those mol numbers to mass, to <u>calculate the mass percent</u>:

  • N₂ ⇒ 0.111 mol * 28 g/mol = 3.108 g N₂
  • H₂ ⇒ 0.196 mol * 2 g/mol = 0.392 g H₂

Mass % N₂ = 3.108/3.49 * 100% = 89.05% ≅ 89%

Mass % H₂ = 0.392/3.49 * 100% = 11.15% ≅ 11%

5 0
3 years ago
Helium has a density of 1.79 x 10-4 g/mL at standard temperature and pressure. A balloon has a volume of 6.3 liters. Calculate t
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9. A student wished to prepare ethylene gas by dehydration of ethanol at 140oC using sulfuric acid as the dehydrating agent. A l
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We have that the the liquid is

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From the question we are told

  • A student wished to prepare <em>ethylene </em>gas by <em>dehydration </em>of ethanol at 140oC using sulfuric acid as the <em>dehydrating </em>agent.
  • A low-boiling liquid was obtained instead of ethylene.
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<h3>Ethylene formation</h3>

Generally the equation is

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Therefore

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The product is diethyl ethen

The reaction at 170 ethylene will give

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Therefore

The the liquid is

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For more information on Ethylene visit

brainly.com/question/20117360

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