The ratio of rate of decomposition of ozone to get molecular oxygen at 50 o C a n d 25 o C has to be determined. Concept Introduction: The temperature dependence of rate constant can be explained through Arrhenius equation. k = A e − E a R T Where k is the rate constant, A is the frequency factor, E a is the activation energy, R is the universal gas constant and T is the temperature.

Question

Using reaction free energy to predict equilibrium composition Consider the following equilibrium: 2NH3 (g) = N2 (g) +3H₂ —N2 (g) AGº = 34. kJ Now suppose a reaction vessel is filled with 4.19 atm of ammonia (NH3) and 9.94 atm of nitrogen (N2) at 378. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NH 3 tend to rise or fall? ☐ x10 fall Х Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of NH 3 will tend to rise, can that be changed to a tendency to fall by adding H₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H₂ needed to reverse it. Round your answer to 2 significant digits. yes no atm 00. 18 Ar 무ㅎ ?

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Question

Chapter 11, Problem 46QRT

Interpretation Introduction

Interpretation:

The ratio of rate of decomposition of ozone to get molecular oxygen at 50oC and 25oC has to be determined.

Concept Introduction:

The temperature dependence of rate constant can be explained through Arrhenius equation.

k=A e−EaRT

Where k is the rate constant, A is the frequency factor, Ea is the activation energy, R is the universal gas constant and T is the temperature.

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