I have the answer for these problems, but I need a clear steps explaination. Can
ID: 1044401 • Letter: I
Question
I have the answer for these problems, but I need a clear steps explaination. Can expert help me out please?
1. The solubility of silver bromide is greater in 0.10 M NaBr than in pure water. True or false? False correct answer why please explain step by step 2. For CO2(g)-CO2(aq), is the entropy change positive or negative? Negative correct answer why please explain step by step . For the reaction 2C(s)2H2()C2H4(g) AH+52.3 klxmol1and AS-53.07 JxK-'xmol 1 at 298 K. This reaction will be spontaneous at: a) no temperature. Correct awswer Why please explain step by step b) all temperatures. c) temperatures below 985 K. d) temperatures above 985 K. e) temperatures below 1015 K.Explanation / Answer
1) AgBr is a weak electrolyte which is partially soluble in water and its solubility decreases in NaBr solution due to common ion effect
AgBr(s) ====== Ag+(aq)+ Br-(Aq)
NaBr(s) ===== Na+(aq) + Br-(aq)
In NaBr solution, the concentration of Br- increases and shifts the reaction backward according to Lechatilier's principle and hence the solubility of AgBr decreases
2) When CO2 gas is dissolved in water, the disorderness of CO2 decreases andn hence the entropy change is negitive
dS = S products - S reactants
The entropy of substances increases with physical states as Solid < Liquid < Gas
3) A reaction becomes spontaneous if the enthalpy of the reaction is negitive and entropy is positive from the Gibbs free energy expression
dG = dH - TdS
If dH = -ve and dS = +ve, reaction the dG becomes -ve and hence the process becomes spontaneous at all T