[[alternative]]An investigation on senior high school studentds' misconceptions of applying Le chatelier's priciple under heterogeneous systems on chemical equilbrium.

[[abstract]]AN INVESTIGATION ON SENIOR HIGH SCHOOL STUDENTS’ MISCONCEPTIONS OF APPLYING LE CHATELIER’S PRINCIPLE UNDER HETEROGENEOUS SYSTEMS ON CHEMICAL EQUILIBRIUM. Lee, Shih-Feng Abstract The study was aimed at investigating the misconceptions of applying Le chatelier’s principle under heterogeneous chemical equilibrium systems for senior high school students in Taiwan. Three hundred and thirty-two 12th grade students in Taoyuan who had studied chemical equilibrium participated in the study. A two-tier test was developed based on the analysis of students’ answers on an open-ended test. There are 50 multiple- choice items, including seven central concepts, where the content knowledge was examined in the first tier and students’ understanding of that knowledge in the second. The test was validated by four senior high school teachers who possessed profound professional chemistry knowledge; The reliability (KR-20) is 0.81. Data were analyzed through descriptive statistics and pearson product-moment correlation. The results indicated a list of 41 patterns of misconceptions underlying misuse of Le chatelier’s principle, 19 of which are identified in literature, whereas 22 of them are unique to this research. The most significant key-miconceptions revealed by the study are: 1.Whatever concentration of reactant may change, the rate of the forward (or reverse) reaction on initial chemical equilibrium should be equal to the rate of the forward (or reverse) reaction on final chemical equilibrium. 2.When insolube salt is dissolved in pure water to form a saturated solution, an equilibrium is established between the solid and its ions in solution. The student thought all the insoluble salt could be dissolved, which could change the solubility equilibria.