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stich3 [128]
3 years ago
9

Nitrogen dioxide decomposes at 300°C via a second-order process to produce nitrogen monoxide and oxygen according to the followi

ng chemical equation.
2 NO2(g) → 2 NO(g) + O2(g).
A sample of NO2(g) is initially placed in a 2.50-L reaction vessel at 300°C. If the half-life and the rate constant at 300°C are 11 seconds and 0.54 M-1 s-1, respectively, how many moles of NO2 were in the original sample?

I just need an idea on how to approach this problem. ...?
Chemistry
1 answer:
qaws [65]3 years ago
4 0
This problem can be simplified by assuming that the reaction took place in a rigid vessel, that is, the volume is held constant. It is also safe to assume that the reaction is isothermal. The first step here is to derive an expression for the dependency of the reactant concentration with time. Since it is stated that the reaction is second order we start with

-dC/dt = k C^2

where

C is the amount of reactant (NO2)
t is time 
k is the reaction rate constant

The negative sign indicates that the concnetration is decreasing with time. Solving the equation, we get

1/Co - 1/C = kt

where Co is the initial amount of NO2

Now we are given the half life which is the time in which the amount of NO2 is halved, that is, C = 0.5Co. Therefore we can solve the initial amount of NO2 (Co) by substituting t = 11 s, k = 0.54 M-1s-1 and C = 0.5Co

Hope this helps
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The molar heat of vaporization of water is 40.7kJ/mol. How much heat must be absorbed to convert 50.0 grams of liquid water at 1
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During a phase change the temperature does not change since all of the heat is being absorbed in order to break the intermolecular forces.  Due to that, the formula will not need to have T in it and is actually q=nΔH(v).
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The atomic theory proposed by dalton has been
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What did Dalton's atomic theory contribute to science?

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3 years ago
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Explanation:

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Read 2 more answers
A solution contains 35 grams of KNO3 dissolved in 100 grams of water at 40°C. How much more KNO3 would have to be added to make
Marta_Voda [28]

Answer:

32g

Explanation:

potassium nitrate has solubility of about 67g per 100g of water at 40°C, which means that potassium nitrate solution will contain 67g of dissolved salt for every 100g of water.

since at this temperature, our solution contains  35g of potassium nitrate 100g  of water. The solution will be unsaturated because of the less potassium nitrate.

to make saturated solution,

mass of potassuim nitrate = 67g - 35g

= 32g

which means dissolving another  32g  of potassium nitrate in solution at 40 °C will make saturated solution.

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