Question 1)
NH4Cl(s)<--->NH3(g) + HCl(g) Delta H=176kJ (per mol HCl)
For the following actions, indicate whether the action causes net reaction from left to right---->, right to left
Action:
The Temperature is increased=
Some NH3 is added=
The equilibrium mixture is transferred to a larger reaction vessel=
Question 2=
Write down Mass balance and charge balance equations for 0.100 mol L-1 NaC2O2O4(aq)
Also,
Question:
What is the value of the equilibrium constant Kc for the reaction below?ASSUME TEMP is 25oC.
HF(aq) +NH3(aq)<-->NH4F(aq)
Also,
Question:A chemist can demonstrate that a reaction, A--> products, is second-order in a few different ways.Two methods are outlined below.PUT IN the missing information for each method.
METHOD #1=Prepare a graph of ___________ versus ____________to show that a linear plot is obtained.The slope of this plot is equal to__________.
METHOD #2=Divide t(3/2) by t(1/2) to show that this ratio is equal to _______________, as it should be for second-order reaction.
Question=
Data:
A=0.10 mol L-1 HCl(aq)
B=0.10 mol L-1 NaOH(aq)
C=0.10 Mol L-1 HNO3(aq)
D=0.10 mol L-1 CH3COOH(aq)
-In which solution(s) is the solubility of AgCl less than the solubility in pure water?
-In which solution(s) is the solubility of Ca(OH)2 greater than the solubility in pure water?
-Adding 1.0 mol of Pb(NO3)2 to 1.0 L of which solution gives the solution with the lowest concentration of Pb2+?