jagdishkumar

The decomposition of ammonia on a tungsten surface at 1100 °C

NH_3-----.>1/2 N₂ + 3/2 H₂

is zero order in NH₃.

In one experiment, when the initial concentration of NH₃ was 1.49×10^-2 M, the concentration of NH₃ dropped to 2.68×10^-3 M after 2.68×10³ secondshad passed.

Based on these data, the rate constant for the reaction is M s^-1.

The zero-order decomposition of ammonia on a hot tungsten surface proceeds according to 2 NH3(g) → N2(g) + 3 H2(g).

The reaction has a half-life of 2.40 × 10 seconds when the initial ammonia concentration is 2.00 M. How long does it take for the concentration of ammonia to decrease from 2.00 M to 1.16 M?
t=____ seconds

The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation

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

The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation.

1. The effects of industrialization were widespread. Please explain at least 3 effects of industrialization around the globe. 

2. Local, national, and international organizations continue to form, united by a common desire to protect our world. Please identify two different types of organizations formed with a common goal of environmentalism and briefly explain the strategies employed by the groups. 

3. Identify 4 of the common features of sustainable design. Please briefly explain each feature. 

4. Our world faces many different challenges due to human interaction with the environment. Please identify at least 4 of our current challenges and briefly explain the significance of each problem. 

In the Haber-Bosch process, nitrogen and hydrogen gas arereacted under high temperature (500 degrees C) and pressure (200atm) to form ammonia gas (NH3) according to the followingequation:

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

If 10600 L H2 gas is reacted with an excess of N2 gas at 200 atmand 500 degrees Celsius, how many moles of ammonia gas would beproduced assuming a 15% yield?

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?