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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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blondinia [14]

2, 4, 1

Explanation:

We have the following chemical reaction:

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So the balanced chemical equation is:

2 Ag₂O → 4 Ag + O₂

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6 0
3 years ago
What period is the atom in?
lys-0071 [83]
It is in period 3
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6 0
3 years ago
The equilibrium constant for the gas phase reaction N2 (g) + O2 (g) ⇌ 2NO (g) is Keq = 4.20 ⋅ 10-31 at 30 °C. At equilibrium, __
pychu [463]

Answer:

At equilibrium, reactants predominate.

Explanation:

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Keq = \frac{[NO]^{2}}{[O_{2} ][N_{2}]}

Since the equilibrium constant is Keq = 4.20x10-31 the concentration of reactants O2 and N2 must be much higher than products to obtain such a small number as  4.20x10-31 at the equilibrium. Hence, at equilibrium reactants predominate.

5 0
3 years ago
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Sodium thiosulfate, na2s2o3, is used as a "fixer" in black and white photography. identify the reducing agent in the reaction of
aev [14]
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8 0
3 years ago
If kc = 7.04 × 10-2 for the reaction: 2 hbr(g) ⇌h2(g) + br2(g), what is the value of kc for the reaction: 1/2 h2(g) + 1/2 br2 ⇌h
Kay [80]
At the first reaction when 2HBr(g) ⇄ H2(g) + Br2(g)
So Kc = [H2] [Br2] / [HBr]^2
7.04X10^-2 = [H2][Br] / [HBr]^2

at the second reaction when 1/2 H2(g) + 1/2 Br2 (g) ⇄ HBr
Its Kc value will = [HBr] / [H2]^1/2*[Br2]^1/2
we will make the first formula of Kc upside down:
1/7.04X10^-2 = [HBr]^2/[H2][Br2]
and by taking the square root: 
∴ √(1/7.04X10^-2)= [HBr] / [H2]^1/2*[Br]^1/2
∴ Kc for the second reaction = √(1/7.04X10^-2) = 3.769 
7 0
3 years ago
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