CO

CO: 4 Balance chemical equations, calculate the molar mass of all compounds in the reaction, and demonstrate how mole ratios play a role in stoichiometry. combustion of methane ( CH 4 ) in oxygen ( O 2 ) to form carbon dioxide ( CO 2 ) and water ( H 2 O ). CH 4 +2 O 2 → CO 2 +2 H 2 O CH 4 : Carbon has a molar mass of 12.01 g/mol Hydrogen has a molar mass of 1.01 g/mol1.01g/mol CH 4 molar mass = 12.01+4×1.01=16.05 g/mol O 2 : Oxygen is a diatomic molecule; molar mass is 2×16.00=32.00 g CO 2 : Carbon molar mass = 12.01 g/mol Oxygen molar mass of 16.00 g/mol, molar mass of CO 2 is 12.01+2×16.00=44.01 g/mol H 2 O : Hydrogen molar mass = 1.01 g/mol Oxygen molar mass =16.00 g/mol H 2 O is 2×1.01+16.00=18.02 g/mol 1 mole of CH 4 reacts with 2 moles of O 2 to produce 1 mole of CO 2 and 2 moles of H 2 O . 1 mole of methane = 2 moles of oxygen Exp. 3 mol of (CH4) to balance equation you need 3 x 2+6 moles of O2. Product= 3×1=3moles of carbon dioxide ( CO 2 ) and 3×2=6 moles of water ( H 2 O ). Week(s): 3, 8 CO: 5 Predict how a change in one or more of the parameters of a gas alters dependent gas parameters such as pressure, volume, or temperature. Changes in the parameters of a gas can have significant effects on other dependent gas parameters, as described by the gas laws. The three primary gas laws are Boyle's Law, Charles's Law, and Gay-Lussac's Law, and they describe the relationships between pressure (P), volume (V), and temperature (T) of a gas when one or more of these parameters change while the others are held constant. example using Boyle's Law. You have a sealed container filled with a certain amount of gas at a constant temperature. Initially, the pressure inside the container is 2 atm, and the volume is 4 L. According to Boyle's Law, P ∝1/ V , pressure is inversely proportional to volume at constant temperature.

If you decrease the volume of the container to 2 L while keeping the temperature constant. Using Boyle's Law, we can calculate the new pressure: P 1 ⋅ V 1 = P 2 ⋅ V 2 (2 atm) ⋅ (4 L)= P 2 ⋅ (2L) P 2 =(2atm) ⋅ (4L) /2L P 2 =4atm So, when the volume is reduced from 4 L to 2 L while the temperature remains constant, the pressure within the container rises from 2 atm to 4 atm. This example explains how changes in one parameter (volume) impact another one (pressure) using Boyle's Law. Week(s): 4, 8 CO: 6 Calculate the concentration and volume of a solution given solute and solvent parameters. Example: You have 50 grams of sodium chloride (NaCl) dissolved in water to make a solution. You want to find out the concentration of the solution and the volume of the solution. Calculate the number of moles of solute (NaCl): Sodium (Na) molar mass = 22.99 g/mol, chlorine (Cl) molar mass = 35.45 g/mol. NaCl = 22.99 g/mol + 35.45 g/mol = 58.44 g/mol moles= mass/molar mass moles=50 g/58.44 g/moL moles≈0.855 mol Calculate the concentration of the solution: Concentration= moles of solute/ volume of solution Concentration=0.855 mol/ V L Calculate the volume of the solution: V = moles of solute /Concentration