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Nutka1998 [239]
3 years ago
12

In the reaction, A -----> Products, the rate constant is 3.6 x 10^−4 s−1. If the initial concentration of A is 0.548 M, what

will be the concentration of A (in M) at t = 99.2 s?
Only enter the numerical value with three significant figures in the answer . Do NOT type in the unit (M).
Chemistry
1 answer:
swat323 years ago
5 0

Answer:

0.529

Explanation:

Let's consider the reaction A → Products

Since the units of the rate constant are s⁻1, this is a first-order reaction with respect to A.

We can find the concentration of A at a certain time t ([A]_{t}) using the following expression.

[A]_{t}=[A]_{0}.e^{-k\times t}

where,

[A]₀: initial concentration of A

k: rate constant

[A]_{t}=0.548M.e^{-3.6\times 10^{-4}s^{-1}\times 99.2s }

[A]_{t}=0.529 M

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Explanation:

The given data is as follows.

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                 = 3.03975 \times 10^{5} Pa

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As relation between work, pressure and change in volume is as follows.

                  W = P \times \Delta V

or,                W = P \times (V_{2} - V_{1})

Therefore, putting the given values into the above formula as follows.

                  W = P \times (V_{2} - V_{1})

                      = 3.03975 \times 10^{5} Pa \times (15 \times 10^{-3} m^{3} - 9 \times 10^{-3} m^{3})

                      = 1823.85 Nm

or,                   = 1823.85 J

As internal energy of the gas \Delta E is as follows.

                     \Delta E = Q - W

                                  = 800 J - 1823.85 J

                                  = -1023.85 J

Thus, we can conclude that the internal energy change of the given gas is -1023.85 J.

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A weak base is one that does not ionize completely in solution. As such, a weak base will have a very low base dissociation constant Kb reflecting its minimal dissociation in solution.

The question is incomplete hence we are are unable to work out the equilibrium but in solution it will look like this;

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Learn more about weak base: brainly.com/question/4131966

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