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Kamila [148]
3 years ago
11

Carbon disulfide, a poisonous, flammable liquid, is an excellent solvent for phosphorus, sulfur, and some other nonmetals. A kin

etic study of its gaseous decomposition reveals these data: Experiment Initial [CS2] (mol/L) Initial Rate (mol/L·s) 1 0.100 2.7 × 10−7 2 0.080 2.2 × 10−7 3 0.055 1.5 × 10−7 4 0.044 1.2 × 10−7 (a) Choose the rate law for the decomposition of CS2
Chemistry
2 answers:
ipn [44]3 years ago
6 0

Answer:

Rate law: = k[CS_2]^1

Explanation:

Given:

t               [CS_2]

0.100            2.7 \times 10^{-7}

0.080          2.2 \times 10^{-7}

0.055         1.5\times 10^{-7}

0.044         1.2\times 10^{-7}

Rate law for the given reaction: k[CS_2]^n

Where, n is the order of the reaction.

Divide rate 1 with rate 3

\frac{0.100}{0.055} =\frac{k[CS_2 (1)]^n}{k[CS_2 (3)]^n} \\\frac{0.100}{0.055} =\frac{k[2.7 \times 10^{-7}]^n}{k[1.5\times 10^{-7}]^n}\\1.81=[1.8]^n\\ n=1

So, rate law = k[CS_2]^1

Maksim231197 [3]3 years ago
3 0

Answer:

r=-3.73x10^{5}s^{-1} [CS_2]

Explanation:

Hello,

In this case, a linealization helps to choose the rate law for the decomposition of CS₂ as it is generalized via:

r=-k[CS_2]^{n}

Whereas n accounts for the order of reaction, which could be computed by linealizing the given data using the following procedure:

-ln(r)=ln(k[CS_2]^{n})\\-ln(r)=ln(k)+ln([CS_2]^{n})\\-ln(r)=ln(k)+n*ln([CS_2])

Therefore, on the attached picture you will find the graph and the lineal equation wherein the slope is the order of the reaction and the <em>y</em>-axis intercept the natural logarithm of the rate constant. In such a way, the order of reaction is 1 and the rate constant is:

ln(k)=12.83\\k=exp(12.83)\\k=3.73x10^{5}s^{-1}

Best regards.

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I hope it will help you.

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B

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How do you work out question 1a?
Sliva [168]

Answer:

-125 kJ

Explanation:

You calculate the energy required to break all the bonds in the reactants. Then you subtract the energy to break all the bonds in the products.

                     H₂C=CH₂   +    H₂ ⟶    H₃C-CH₃

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The formula relating ΔHrxn and bond dissociation energies (D) is

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(Note: This is an exception to the rule. All other thermochemical reactions are “products – reactants”. With bond energies, it’s “reactants – products”. The reason comes from the way we define bond energies.)

<em>For the reactant</em>s:

Σ(Dreactants) = 4 × 413 + 1 × 612 + 1 × 436 = 2700 kJ

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2CO + O2 --&gt; 2CO2
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10 L of CO₂.

Explanation:

The balanced equation for the reaction is given below:

2CO + O₂ —> 2CO₂

From the balanced equation above,

2 L of CO reacted to produce 2 L of CO₂.

Finally, we shall determine the volume of CO₂ produced by the reaction of 10 L CO. This can be obtained as follow:

From the balanced equation above,

2 L of CO reacted to produce 2 L of CO₂.

Therefore, 10 L of CO will also react to produce 10 L of CO₂.

Thus, 10 L of CO₂ were obtained from the reaction.

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