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Stels [109]
2 years ago
10

What is the molarity of a solution in which 58g of nacl are dissolved in 1.0 l of solution

Chemistry
1 answer:
Lady_Fox [76]2 years ago
7 0

Hey there :

Molar mass of NaCl = 58.44 g/mol

Number of moles :

n = mass of solute / molar mass

n = 58 / 58.44

n = 0.9924 moles of NaCl

Volume = 1.0 L

Therefore:

Molarity = number of moles / volume ( L )

Molarity = 0.9924 / 1.0

Molarity = 0.9924 M

Hope that helps!

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At 700 K, the reaction 2SO2(g) + O2(g) <====> 2SO3(g) has the equilibrium constant Kc = 4.3 x 106. At a certain instant, f
nadya68 [22]

Answer:

The system is not in equilibrium and will evolve left to right to reach equilibrium.

Explanation:

The reaction quotient Qc is defined for a generic reaction:

aA + bB → cC + dD

Q=\frac{[C]^{c} *[D]^{d} }{[A]^{a}*[B]^{b}  }

where the concentrations are not those of equilibrium, but other given concentrations

Chemical Equilibrium is the state in which the direct and indirect reaction have the same speed and is represented by a constant Kc, which for a generic reaction as shown above, is defined:

Kc=\frac{[C]^{c} *[D]^{d} }{[A]^{a}*[B]^{b}  }

where the concentrations are those of equilibrium.

This constant is equal to the multiplication of the concentrations of the products raised to their stoichiometric coefficients divided by the multiplication of the concentrations of the reactants also raised to their stoichiometric coefficients.

Comparing Qc with Kc allows to find out the status and evolution of the system:

  • If the reaction quotient is equal to the equilibrium constant, Qc = Kc, the system has reached chemical equilibrium.
  • If the reaction quotient is greater than the equilibrium constant, Qc> Kc, the system is not in equilibrium. In this case the direct reaction predominates and there will be more product present than what is obtained at equilibrium. Therefore, this product is used to promote the reverse reaction and reach equilibrium. The system will then evolve to the left to increase the reagent concentration.
  • If the reaction quotient is less than the equilibrium constant, Qc <Kc, the system is not in equilibrium. The concentration of the reagents is higher than it would be at equilibrium, so the direct reaction predominates. Thus, the system will evolve to the right to increase the concentration of products.

In this case:

Q=\frac{[So_{3}] ^{2} }{[SO_{2} ]^{2}* [O_{2}] }

Q=\frac{10^{2} }{0.10^{2} *0.10}

Q=100,000

100,000 < 4,300,000 (4.3*10⁶)

Q < Kc

<u><em> The system is not in equilibrium and will evolve left to right to reach equilibrium.</em></u>

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3 years ago
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Answer: YES!

Explanation:

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3 0
2 years ago
What is the molality of chloride ions in an aqueous solution of magnesium chloride for which xmgcl2 is 0.01?
AfilCa [17]
MgCl₂ ---> Mg(2+) + 2Cl(-)
0,01-x.............x.............2x

MgCl₂ ---> Mg(2+) + 2Cl(-)
0,01-x.............x.............2x
0...................0,01.......0,02

The molality of chloride ions is 0,02M.
8 0
3 years ago
Fe (s) + Pb(NO3), (aq) —&gt; ___<br><br> Type of reaction: _____
OlgaM077 [116]

Answer:

lead , chemical

Explanation:

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William measures a test tube and finds that the mass of the test tube is 5g. He places the lone reactant in the test tube and fi
iogann1982 [59]

86 percent is the percent yield for this experiment if he expected to produce 5g of product.

Explanation:

Given that:

mass of test tube = 5 grams

mass of test tube + reactant is 12.5 grams

mass of reactant = ( mass of test tube + reactant ) - (mass of test tube)

mass of reactant = 12.5 -5

                             = 7.5 grams

when 7.5 grams of reactant is heated mass of test tube was found to be 9.3 grams.

so mass of product formed = 9.3 - 5

                                             = 4. 3 grams of product is formed (actual yield)

However, he expected the product to be 5 grams (theoretical yield)

Percent yield = \frac{actual yield}{theoretical yield} x 100

          putting the values in the formula:

percent yield = \frac{4.3}{5} x 100

                     = 86 %

86 percent is the percent yield.

5 0
3 years ago
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