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Chemistry
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11 Dec 2019

The decomposition of ammonia is found to be a first-order process with a rate constant k=0.0033s-1

2NH3 (g) ---> N2 (g) + 3H2 (g)

A) If the concentration of ammonia is initially 0.500 moles/L, then how long will it take for the concentration to decrease to 0.100 moles/L

B) What is the initial concentration of ammonia if the concentration is measured and found to be 0.25 moles/L after 30 seconds

C) What is the half life for this reaction?

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Related questions

Consider the following reaction:

N2(g) + 3H2(g) ? 2NH3(g)


In a given experiment, 1.00 moles of N2(g) and 4.52 moles of H2(g)were placed in a 3.10 L vessel.
At a particular temperature, the equilibrium concentration of NH3is found to be 0.345 M.
Given this information, determine the numerical value of K for thisreaction, at this temperature.
(If you want to enter your answer in scientific notation, use theformat as shown below:
2.5 x 10-3 = 2.5E-3)

K =

For the reaction: 2POCl3(g)2PCl3(g) + O2(g) ΔH = +508kJ

Complete the table below by writing: increase, decrease, or noeffect.

Kp

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The mixture is cooled from 100 oC to 85oC

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Adding a catalyst

) A 3.000-L flask isinitially filled with 3.00 mol of HI(g) at 448oC.

The reaction is2HI(g) H2(g) +I2(g) Kc = 0.198 at 448 oC.

Calculate the equilibriumconcentrations of H2, I2, and HI in moles perliter at

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A 50.0 L vessel contains1.00 mol N2, 3.00 mol H2, and 0.500 molNH3.

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3) C (s) +H2O(g) CO(g) +H2(g)

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