Answer Happy

Consider the folowing phase reaction NO (0) + N 0(0) + 3 NO() thing data from Appendix of your textbook calculate the temperature, at which this reaction will be at equilibrium under standard conditions (0) and choose whether AG will increase, decrease or not change with increasing temperature from the pulldown menu 1.- k and ac waSelod-with increasing temperature For each of the temperatures listed below calitate ac for the reaction above, and select from the pulldown menu whether the reaction under standard conditions will be spontaneous nonpontaneous, ornar equilibrium (rear equilibrium" means that is within 5 K of T). (a) ALT=454KG mol, and the reaction is see under standard conditions (AT-2008 kime, and the reaction is Soled under standard conditions ALT 162KG- mol, and the reaction is al Mundar standard conditions

Consider the following data. 2 C(s) + H2(9) = C2H2(9) CO2(9) = C(s) + O2(9) 2 H20(I) = 2 H2(g) + O2(9) ΔΗ = +226.8kg AH = +393.5 ka AH = +571.7 kJ Use Hess's law to calculate AH for the reaction below. 2 CH2(9) +5 02(9) = 4CO2() + 2 H2001) ΔΗ = ka

A buffer solution contains 0.60 mol of hypobromous acid (HBrO) and 0.67 mol of sodium hypobromite (NaOBr) in 6.10 L. The K, of hypobromous acid (HBrO) is Ky = 2.5e-09. (a) What is the pH of this buffer? pH = (b) What is the pH of the buffer after the addition of 0.30 mol of NaOH? (assume no volume change) pH = (c) What is the pH of the original buffer after the addition of 0.57 mol of Ht? (assume no volume change) pH =