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krek1111 [17]
2 years ago
6

14. Calculate the mass in grams of oxygen required to react completly with 0.75 moles of Aluminum.

Chemistry
1 answer:
cluponka [151]2 years ago
8 0
  • 3mols of O_2 react with 4mol of Al
  • 3/4=0.75mol O_2 react with 1mol of Al

Moles of O_2:-

  • 0.75(0.75)
  • 0.5625mol

Mass of O_2:-

  • moles(Molar mass)
  • 0.5625(32)
  • 18g

Option B

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The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way:
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Explanation:

(a)  As the given chemical reaction equation is as follows.

           OCl^{-} + I^{-} \rightarrow OI^{-1} + Cl^{-1}

So, when we double the amount of hypochlorite or iodine then the rate of the reaction will also get double. And, this reaction is "first order" with respect to hypochlorite and iodine.

Hence, equation for rate law of reaction will be as follows.

              Rate = K \times [OCl^{-}] \times [l^{-}]

(b)  Since, the rate equation is as follows.

                    Rate = K [OCl^{-}][l^{-}]

Let us assume that ([OCl^{-}] = [l^{-}])

Putting the given values into the above equation as follows.

             1.36 \times 10^{-4} = K \times (1.5 \times 10^{-3})^2

            1.36 \times 10^{-4} = K \times (2.25 \times 10^{-6})

                   K = \frac{1.36 \times 10^{-4}}{2.25 \times 10^{-6}}

                      = 60.4 M^{-1}sec^{-1}

Hence, the value of rate constant for the given reaction is 60.4 M^{-1}sec^{-1} .

(c) Now, we will calculate the rate as follows.

                Rate = K [OCl^{-}][l^{-}]

                         = 60.4 \times (1.8 \times 10^{3}) \times (6.0 \times 10^{4})

                        = 6.52 \times 10^{5}

Therefore, rate when [OCl^{-}] = 1.8 \times 10^{3} M and [I^{-}]= 6.0 \times 10^{4} M is  6.52 \times 10^{5}.

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The Earth's biosphere is consists of
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The decomposition of acetaldehyde is a second order reaction with a rate constant of 4.71 10−8 L/mol/s. What is the instantaneou
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Answer: Rate of decomposition of acetaldehyde in a solution is 1.45\times 10^{-14}mol/Ls

Explanation:

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

For a reaction : A\rightarrow products

Rate=k[A]^x

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Thus rate of decomposition of acetaldehyde in a solution is 1.45\times 10^{-14}mol/Ls

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