Which of the following mixtures creates a buffer solution?
A) 10.0 ml of 0.10M NaOH, 10.0ml of 0.10M HF
B) 20.0 ml of 0.10M NaOH, 15.0ml of 0.10M HF
C) 15.0 ml of 0.10M NaOH, 20.0ml of 0.10M HF
D) 10.0 ml of 0.10M NaOH, 5.0ml of 0.20M HF
Well I new that A and D were not the answers because they are essentially the same thing. The answer is C but I'm not exactly sure why.
Consider the system at equilibrium:
2SO2(g) + O2(g) <--> 2SO3(g)
for which (delta)H < 0. Which change(s) will increase the yield of SO3(g)?
I. Increasing the temperature
II. Increasing the volume of the container
A) I only
B) II only
C) Both I and II
D) Neither I nor II
For this one, I new that the second statement would not be true because that would decrease the pressure, which favors the side with more moles of gas, in this case the reverse reaction. So I cancelled out choices B and C. But I'm not very clear on how temperature affects an endothermic reaction. I put A but the answer was D. If this reaction was exothermic, would the answer be A?
How much heat is required to convert 5.0g of ice at -10.0 C to liquid water at 15.0 C? (assume heat capacities are independent of temperature.)
Enthalpy of fusion: 6.00 kJ/mol
Specific heat capacity of ice: 37.8 J/mol
Specific heat capacity of water: 76.0 J/mol
A) 4.2 x 10^2 J
B) 2.1 x 10^3 J
C) 9.3 10^3 J
D) 3.8 x 10^4 J
I'm in AP Chem right now and my teacher never really brushed over heat capacities at all. I put D, but the answer was B. Can someone help me out on this?