Consider a 0.010 M Sr(OH)2, calculate the pH of this solution. Show your solution in your scratch paper that needs to be uploaded. No solution no points. Observe significant figure rules.

The Haber-Bosch process is the main industrial route to production of ammonia and is written as: N2(g) +3H2(g) ↔ 2NH3(g) with a ΔH° for the reaction being -92.4 kJ/mol. How would a decrease in the volume of the container affect the equilibrium ? Which direction, if any, will the reaction go to re-establish the equilibrium?

If I mix an equimolar (same amount of moles) amount of a weak acid (HCN) and a strong base (NaOH), what will be the pH of the combined solution after the reaction (pH >, < or = 7) ?   

Kc is equal to 0.28 for the following reaction at 900 °C: CS2(g)+4H2(g) ⇌ CH4(g) + 2H2S(g) What is KP at this temperature?

Consider a sealed vessel containing the H2, I2, and HI gases at equilibrium according to the equation: 2HI(g) ↔ H2(g) + I2(g) with a ∆H°reaction = -299 kJ/mol. Predict how the following changes affect the equilibrium (forward, reverse, no change). Addition of a catalyst

Consider the equilibrium constant Kc for the reaction: N2O4(g) ↔ 2NO2(g) is 0.211 at 100°C. What is the value for the equilibrium constant is the reaction is balanced as ½ N2O4(g) ↔ NO2(g) ? Show your solution in your scratch paper that needs to be uploaded. No solution no points. Observe significant figure rules.  

An ecosystem includes:

Fast-moving rivers usually have:

Which violates Hardy-Weinberg conditions?

Binary fission is a form of: