Chemistry 107 Exam Questions – 40 Exam Questions and 100% Correct Answers on Solutions, Colligative Properties, and Thermochemistry (Chem107)

This document contains approximately 40 exam questions with 100% verified answers designed to help students prepare for Chemistry 107 exams in a university General Chemistry course. The material provides a structured review of solution chemistry and thermodynamics concepts, including concentration units such as molarity, molality, mole fraction, mass percent, and parts per million (ppm). It also explains how temperature affects solution concentration and discusses key calculation methods used in chemistry problems involving solute–solvent relationships and solution composition. These topics are presented in a clear question-and-answer format to help students quickly review formulas and definitions commonly tested in chemistry exams. The document also covers important laws and principles used in solution chemistry, including Henry’s Law for gas solubility in liquids, Raoult’s Law for vapor pressure in solutions, and the theory of colligative properties such as freezing point depression. Detailed explanations are provided for equations like ΔT = iKf m and how the van’t Hoff factor affects the number of dissolved particles in a solution. Additional sections review osmotic pressure calculations, electrolyte vs. nonelectrolyte behavior, and how the number of dissolved ions influences physical properties such as boiling point elevation and freezing point depression. Further topics include thermochemistry calculations using formulas such as q = mCΔT and q = nΔH, properties of crystalline and amorphous solids, and crystal lattice structures including simple cubic, face-centered cubic, and body-centered cubic unit cells. The document also discusses metallic properties, band gap theory for conductors, semiconductors, and insulators, as well as concepts related to vapor pressure, critical points, and temperature effects on solubility. These concepts form an essential foundation for understanding physical chemistry behavior and chemical materials. The material aligns with topics commonly taught in General Chemistry II courses and supports learning objectives found in widely used textbooks such as Chemistry: The Central Science by Theodore L. Brown, H. Eugene LeMay, Bruce E. Bursten, and Catherine Murphy, which provide comprehensive coverage of solution chemistry, thermodynamics, and physical properties of matter. This study resource is designed to reinforce lecture material and provide quick revision before midterms, finals, or chemistry exams. This document may be particularly useful for students enrolled in courses such as: Chem107 General Chemistry II College Chemistry II Introductory Chemistry for Science Majors Principles of Chemistry II Fundamentals of Chemical Principles It may benefit students studying in the following programs: Chemistry Biochemistry Biology Pre-medicine Pharmacy Chemical engineering Health sciences Biotechnology Environmental science Keywords: molarity formula, molality formula, mole fraction calculation, mass percent chemistry, ppm concentration chemistry, solution concentration units, henrys law chemistry, gas solubility in liquids, raoults law vapor pressure, colligative properties chemistry, freezing point depression formula, vant hoff factor, osmotic pressure equation, electrolyte vs nonelectrolyte, thermochemistry formulas, q mc delta t equation, enthalpy change calculation, crystalline solids structure, simple cubic unit cell, face centered cubic lattice, body centered cubic structure, band gap theory chemistry, conductors semiconductors insulators, vapor pressure of solutions, critical point chemistry, temperature effect on solubility