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Blababa [14]
3 years ago
12

The second-order rate constant for the following gas-phase reaction is 0.041 1/MLaTeX: \cdotâs. We start with 0.438 mol C2F4 in

a 2.42 liter container, with no C4F8 initially present. C2F4 LaTeX: \longrightarrowâ¶ 1/2 C4F8 What is the half-life (in seconds) of the reaction for the initial C2F4 concentration? Enter to 1 decimal place.
Chemistry
1 answer:
pantera1 [17]3 years ago
3 0

Answer:

134.8 seconds is the half-life (in seconds) of the reaction for the initial C_2F_4 concentration

Explanation:

Half life for second order kinetics is given by:

t_{\frac{1}{2}=\frac{1}{k\times a_0}

Integrated rate law for second order kinetics is given by:

\frac{1}{a}=kt+\frac{1}{a_0}

t_{\frac{1}{2} = half life

k = rate constant

a_0 = initial concentration

a = Final concentration of reactant after time t

We have :

C_2F_4 \longrightarrow \frac{1}{2} C_4F_8

Initial concentration of C_2F_4=[a_o]=\frac{0.438 mol}{2.42 L}=0.1810 mol/L

Rate constant = k = 0.041 M^{-1} s^{-1}

t_{\frac{1}{2}=\frac{1}{k\times a_0}

=\frac{1}{0.041 M^{-1} s^{-1}\times 0.1810 mol/L}

t_{1/2}=134.8 s

134.8 seconds is the half-life (in seconds) of the reaction for the initial C_2F_4 concentration

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Answer:

4804.5 g of SO₂ are needed to the reaction

Explanation:

The reaction to produce sulfuric acid is:

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Ratio is 1:2. 1 mol of oxygen needs 2 moles of sulfur dioxide in order to react. We can propose this rule of three.

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How many moles of PC15 can be produced from 58.0 g of Cl₂ (and excess<br> P4)?
ludmilkaskok [199]

0.3268 moles of PC15 can be produced from 58.0 g of Cl₂ (and excess

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<h3>How to calculate moles?</h3>

The balanced chemical equation is

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The amount of clorine is n(Cl_{2}) = m(Cl_{2})/M(Cl_{2}) = 58/70.906 = 0.817 mol

The stoichiometric reaction,shows that

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n(PCl_{5}) = 4*0.817/10 = 0.3268 mol

To know more about stoichiometric reaction, refer:

brainly.com/question/14935523

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Explanation:

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Answer:

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a quantity of gas has a volume of 400.0 mL when confined under a pressure of 600.0mm Hg. what will be the new volume of the gas
Alex787 [66]

Answer:

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Explanation:

Given data

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For a gaseous sample, there is an inverse relationship between the pressure and the volume. If we consider the gas as an ideal gas, we can find the final volume using Boyle's law.

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3 years ago
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