𝗺𝗼𝗹𝗲 𝗰𝗼𝗻𝗰𝗲𝗽𝘁 — 𝗻𝗼𝘁𝗲𝘀 — ᰔ..pdf

♡mole concept ♡ introduction: 23 ○ a mole is the amount of substance that contains 6.02 x 10 particles of that substance ○ or a mole is the amount of substance (grams) that contains the s...

♡mole concept ♡ introduction: 23 ○ a mole is the amount of substance that contains 6.02 x 10 particles of that substance ○ or a mole is the amount of substance (grams) that contains the same number of particles as there are in 12 grams of carbon-12 (these particles can be molecules, ions, etc) 12 the actual number of carbon 12 atoms in 12 grams of C is 6.02 x 23 10 (avogaddro’s constant) it therefore follows that: 23 ○ one mole of an element contains 6.02 x 10 atoms 23 ○ or 1 mole of an ionic compound contains 6.02 x 10 formula units ○ or 1 mole of a covalent compound contains 6.02 x 23 10 molecules molar mass: ○ molar mass (mm) is the mass of one mole of a substance formula:  amount of ions x relative mass eg: ○ H2O = (2 amount of hydrogen ions x 1 relative mass of hydrogen) + (1 -1 amount of oxygen ions x 16 relative mass of oxygen) = 18g/mol ○ Ca(NO3)2 = (1 amount of calcium ions x 40 relative mass of calcium) + (2 amount of nitrogen ions x 14 relative mass of nitrogen) + (6 amount of oxygen ions x 16 relative mass of oxygen) = 164g/mol ○ relative molecular mass (rmm) is the ratio of one mole of a substance compared to 1/12 the mass of a carbon 12 atom relative molecular mass and molar mass are numerically equal, however, molar mass have units of gram per mole, and relative molecular mass does not have a unit relative molecular mass does not have a unit because they cancel each other plotting a mole graph: ○ plotting a graph: -3 concentration/ mol dm time /s 0.0 44 0.2 30 0.4 18 0.6 10  0.8 4 1.0 0 rules for plotting a graph: ○ graph must have a title and scale ○ scale must take more than half of both the y and x axis ○ label the x and y axis, and the unit of measurement must be included ○ fine point pencil must be used ○ points must be identified with a dot and a circle around it ○ the lines that you’re using to plot your graph should not be lighter than your y and x axis conversion: ○ conversion: calculate the number of moles in 6 grams of carbon mass → # of mol ○ 12g of carbon has 1 mol ○ 6g of carbon will have x 12x/12 = 6/12 (cross multiply) = 0.50 mol of carbon calculate the number of moles in 11.7g of NaCl mass → # of mol ○ molar mass of NaCl = (1 x 23) + (1 x 35.5) = 58.5 -1 gmol  58.5g of NaCl has 1 mol 11.7g of NaCl will have x 58.5x/58.5 = 11.7g/58.5 (cross multiply) ○ = 0.20 mol of NaCl calculate the mass of 5 moles of NaOH # of mol → # mass ○ molar mass of NaOH = (1 x 23) + (1 x 16) + (1 x 1) = -1 40 gmol 1 mol of NaOH has 40g 5 mol of NaOH will have x x = 5 x 40 ○ = 200g NaOH -9 calculate the mass of 1.56 x 10 moles of hydrogen (H2) # of mol → # mass ○ 1 mol of H2 has 2g (1 x 2 because it it a diatomic molecule) -9 ○ 1.56 x 10 moles of H2 will have x -9 x = 2 x 1.56 x 10 moles 3.12 x 10-9g of H2  volume of gasses: ○ avogadro's law states that equal volumes of all gasses, under the same conditions of temperature and pressure, contain the same number of molecules 23 molar volume (vm) is the volume occupied by one mole (6.0 x 10 molecules) of a gas this depends on temperature and pressure: ○ at standard temperature & pressure (stp), where temperature is 0 degrees celsius and pressure is 101.3 kPa (1 atmosphere), the volume of one mole of gas is 22.4 cm3 or 22,400 cm3 ○ at room temperature & pressure (rtp), where temperature is 25 degrees celsius and pressure is 101.3 kPa (1 atmosphere), the volume of one mole of gas is 24.0 cm3 or 24,000 cm3 molar volume can be used to convert a given volume of a gas → number of moles, or to convert a given number of moles of a gas → volume two conversions: given volume of gas → number of moles: ○ number of moles = given volume of gas/volume of one mole at stp or rtp (molar volume)  given volume of moles → volume of gas: ○ volume of gas = given volume of moles x volume of one mole at stp or rtp (molar volume) questions: ○ questions: introduction: what is a mole? what does 1 mole of an element contain? what does 1 mole of an ionic compound contain? what does 1 mole of a covalent compound contain? molar mass: what is molar mass? how is molar mass calculated? how do you calculate the molar mass of H₂O? how do you calculate the molar mass of Ca(No₃)₂? what is relative molecular mass (rmm)? does relative molecular mass have units? plotting a mole graph: how is a mole graph plotted? conversion: what is the formula for converting mass to moles? how do you calculate the number of moles in 6 g of carbon?  how do you calculate the number of moles in 11.7 g of NaCl? how do you calculate the mass of 5 moles of NaOH? how do you calculate the mass of 1.56 x 10⁻⁹ moles of H₂? volume of gasses: what does avogadro’s law state? what is molar volume? what is the volume of 1 mole of gas at stp? what is the volume of 1 mole of gas at rtp? how do you convert volume of gas to moles? how do you convert moles to volume of gas?