화학 강의 Stoichiometry ICE Table 빠르게 간단하게 해결 하기 위한 영상입니다. Welcome to our channel! In today's video, we dive into stoichiometry and learn how to use ICE tables to solve problems quickly and efficiently. Stoichiometry is a fundamental concept in chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. We will cover the basics of stoichiometry, including balancing chemical equations. You will also learn what an ICE table is and how it helps in solving stoichiometric problems. ICE stands for Initial, Change, and Equilibrium – a systematic approach to track the concentrations of reactants and products throughout a reaction. By the end of this video, you'll be able to tackle stoichiometry problems with confidence and ease!
화학 강의 Stoichiometry ICE Table 빠르게 간단하게 해결 하기 위한 영상입니다. Welcome to our channel! In today's video, we dive into stoichiometry and learn how to use ICE tables to solve problems quickly and efficiently. Stoichiometry is a fundamental concept in chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. We will cover the basics of stoichiometry, including balancing chemical equations. You will also learn what an ICE table is and how it helps in solving stoichiometric problems. ICE stands for Initial, Change, and Equilibrium – a systematic approach to track the concentrations of reactants and products throughout a reaction. By the end of this video, you'll be able to tackle stoichiometry problems with confidence and ease!
Problem 1: For the reaction N2 + 3H2 → 2NH3, if you start with 1.0 mol of N2 and 3.0 mol of H2, how many moles of NH3 will be formed?
ICE Table:
Initial: [N2] = 1.0 M, [H2] = 3.0 M, [NH3] = 0 M
Change: [N2] = -x, [H2] = -3x, [NH3] = +2x
Since N2 is the limiting reagent, x = 1.0. Thus, [NH3] = 2(1.0) = 2.0 M.
Problem 2: For the reaction 2SO2 + O2 → 2SO3, if you start with 2.0 mol of SO2 and 1.0 mol of O2, how many moles of SO3 will be formed?
ICE Table:
Initial: [SO2] = 2.0 M, [O2] = 1.0 M, [SO3] = 0 M
Change: [SO2] = -2x, [O2] = -x, [SO3] = +2x
Since SO2 is the limiting reagent, x = 1.0. Thus, [SO3] = 2(1.0) = 2.0 M.
Problem 3: For the reaction 2H2 + O2 → 2H2O, if you start with 4.0 mol of H2 and 2.0 mol of O2, how many moles of H2O will be formed?
ICE Table:
Initial: [H2] = 4.0 M, [O2] = 2.0 M, [H2O] = 0 M
Change: [H2] = -2x, [O2] = -x, [H2O] = +2x
Since H2 is the limiting reagent, x = 2.0. Thus, [H2O] = 2(2.0) = 4.0 M.
Problem 4: For the reaction C + O2 → CO2, if you start with 1.0 mol of C and 1.0 mol of O2, how many moles of CO2 will be formed?
ICE Table:
Initial: [C] = 1.0 M, [O2] = 1.0 M, [CO2] = 0 M
Change: [C] = -x, [O2] = -x, [CO2] = +x
Since both reagents are in stoichiometric proportion, x = 1.0. Thus, [CO2] = 1.0 M.
Problem 5: For the reaction N2 + 3H2 → 2NH3, if you start with 0.5 mol of N2 and 1.5 mol of H2, how many moles of NH3 will be formed?
ICE Table:
Initial: [N2] = 0.5 M, [H2] = 1.5 M, [NH3] = 0 M
Change: [N2] = -x, [H2] = -3x, [NH3] = +2x
Since N2 is the limiting reagent, x = 0.5. Thus, [NH3] = 2(0.5) = 1.0 M.