Temperature C 25 °C Write the Ksp expression here: Calculate the Ksp value here (Show work): Volume of Distilled Water (mL) 100 mL Solid: Ag2CO3 Mass of Solid (g) Molarity of Ag+ 100 g Molarity of CO3^(2-) 2.56490 x 10^-4 1.28245 x 10^-4

Compound NH4HCO3(s) NH3(g) CO2(g) H20(E) AG°; (kJ/mol) -665.9 -16.45 -394.4 -237.1 Consider the given reaction: NH3(g) + CO2(g) + H20(4) = NH4HCO3(s) Calculate AG at 298K for this reaction when the pressures of NH3 and CO2 are 0.52 atm and 0.31 atm, respectively. 22.5 kJ -26.7 kJ -13.4 kJ O 13.4 kJ O -22.5 kJ

Please help us with number five in picture. We are getting 1.5 and I'm not sure if they are asking and telling us that .5 is the equilibrium pressure of dinitrogen pentoxide.  Or if .5 is the total.This is not a graded question as it is a practice question . I am 60 years old and helping my son prepare for the AP exam in a few months. We do questions at the back of the textbook by Zumdahl and Zumdahl.  I believe the answer is D but I am getting 1.5

Please help i don't really understand this question.

Consider The Following Reaction M Inbox (208) - eleganceextreme1 X + 05657571&snapshotld=13245488id-563649000&takeld-4bfba59b09f0e5b& X X QSearch this course X References Use the References to access important values if d for this question. *** The equilibrium constant, K,, for the following reaction is 8.46x10 at 298 K: 1 00 NH3(g) + H2Se(g) NH4HSe(s) A-Z Calculate the partial pressure of each gas and the total pressure at equilibrium when 0.469 moles of NHHSe(s) is introduced into a 1.00 L vessel at 298 K. Assume that the volume occupied by the solid is negligible. PNH3 atm atm PH2SE atm Ptotal 6. Equilibrium Calculations with Partial Pressur... : This is group attempt 1 of 5 Next Autosaved at 1:06 PM Back 1:06 PM xa 11 9/24/2019 1 hp delete rt co

Please do both neat and clean correctly otherwise don't do it... Thanks

[Rev Topics] [References] Use the References to access important values if needed for this question. Consider the following reaction where Ke = 6.30 at 723 K. 2NH3 (9) N₂(g) + 3H₂(g) A reaction mixture was found to contain 0.000687 moles of NH3(g), 0.0258 moles of N₂ (g), and 0.0435 moles of H₂(g), in a 1.00 liter container. Calculate Qc. Qc = 1 Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction must run in the forward direction to reach equilibrium. The reaction must run in the reverse direction to reach equilibrium. The reaction is at equilibrium. Submit Answer Retry Entire Group 9 more group attempts remaining Previous Next> ad Exit ? or n er