Problem- The gas arsine, AsH3, decomposes to form solid arsenic and hydrogen gas in the following equilibrium reaction: 2AsH3(g) < --- > 2As(s) + 3H2(g) You inject 280.0 torr of arsine into an evacuated chamber, and measure a total pressure on successive days that does not change and remains at 380.0 torr. You may assume that the gases are ideal and that the temperature remains constant at T = 25.0°C
Part a) What is the equilibrium pressure of the hydrogen gas?
Part b) What are the equilibrium constant K and delta G° for this reaction?
Part c) Next, you rapidly inject an additional 120.0 torr of hydrogen gas into the chamber, disturbing the previously established equilibrium.
What is the reaction quotient Q immediately after this injection? Which direction will the reaction shift (towards reactants, towards products, or neither) and why? Briefly justify your answer with 1-2 sentences.
Please demonstrate the entire work. I am thanking you in advance