Predict whether each of the following transformation leads to an increase or decrease in the entropy of a system. DO THE FOLLOWING DECREASE OR INCREASE IN ENTROPY
a- Br2(l) to Br2(g)
b- I2(g) to I2(s)
c- higher density S(a) to lower density S(B)
d- C (graphite) to C (diamonds)
e- NaCl(s) to NaCl(aq)

A.(nh4)(2co3)is the correct answer 

Ibelieve it’s 1.95m

Reaction involved in present system is :   c12h22o11 + h2o → 2 c6h12o6the reaction system is obeying following rate law:   rate = k[c12h22o11]thus, it is a first order reaction.now, for 1st order reactionrate constant (k) =  given: initial conc. = 3.0 g, final conc. = 2.7 g, t = 2.5 h∴rate constant (k) =  ∴ k = 0.04215 h-1now, for 1st order reaction, half life = 0.693/k = 0.693/0.04215 = 16.4 hthus correct answer is option b