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formulas
| Question | Answer |
|---|---|
| What is the formula for density? | D = m/V |
| How do you calculate mass from density? | m = D × V |
| How do you calculate volume from density? | V = m/D |
| What is the formula for percent error? | % error = |experimental - accepted| / accepted × 100 |
| What is the formula for molarity? | M = mol/L |
| How do you calculate moles from molarity? | mol = M × L |
| How do you calculate volume from molarity? | L = mol/M |
| What is the dilution formula? | M1V1 = M2V2 |
| What is the formula for percent by mass? | % mass = mass solute/mass solution × 100 |
| What is the formula for mass of solution? | mass solution = mass solute + mass solvent |
| What is the formula for percent by volume? | % volume = volume solute/volume solution × 100 |
| What is the formula for parts per million? | ppm = mass solute/mass solution × 1,000,000 |
| What is the formula for moles from mass? | mol = g/molar mass |
| How do you calculate grams from moles? | g = mol × molar mass |
| What is Avogadro's number? | 6.02 × 10^23 particles/mol |
| How do you calculate moles from particles? | mol = particles/(6.02 × 10^23) |
| How do you calculate particles from moles? | particles = mol × (6.02 × 10^23) |
| What is the formula for percent composition by mass? | (mass of element/mass of compound) × 100 |
| What is the formula for heat? | q = mCΔT |
| What does q represent in q = mCΔT? | Heat energy |
| What does m represent in q = mCΔT? | Mass |
| What does C represent in q = mCΔT? | Specific heat |
| What does ΔT represent in q = mCΔT? | Change in temperature |
| What is the formula for change in temperature? | ΔT = Tf - Ti |
| What is the formula for heat of fusion? | q = mHf |
| What is the formula for heat of vaporization? | q = mHv |
| What is the formula for heat of reaction? | ΔH = PEproducts - PEreactants |
| What is the formula for pH? | pH = -log[H+] |
| What is the formula for pOH? | pOH = -log[OH-] |
| What is the relationship between pH and pOH? | pH + pOH = 14 |
| What is the ion product constant for water? | [H+][OH-] = 1 × 10^-14 |
| How do you calculate hydroxide concentration from hydrogen concentration? | [OH-] = (1 × 10^-14)/[H+] |
| How do you calculate hydrogen concentration from hydroxide concentration? | [H+] = (1 × 10^-14)/[OH-] |
| What is the titration formula? | MaVaia = MbVbib |
| What does ia represent in the titration formula? | Number of H+ ions produced by the acid |
| What does ib represent in the titration formula? | Number of OH- ions produced by the base |
| What is the combined gas law? | P1V1/T1 = P2V2/T2 |
| What temperature unit must be used in gas law calculations? | Kelvin |
| How do you convert Celsius to Kelvin? | K = °C + 273 |
| What is the ideal gas law? | PV = nRT |
| What is the Gibbs free energy equation? | ΔG = ΔH - TΔS |
| What is Einstein's mass-energy equation? | E = mc^2 |
| What is the formula for atomic mass? | protons + neutrons |
| How do you calculate neutrons? | mass number - atomic number |
| How do you calculate average atomic mass? | Σ(isotope mass × decimal abundance) |
| What fraction remains after one half-life? | 1/2 |
| What fraction remains after two half-lives? | 1/4 |
| What fraction remains after three half-lives? | 1/8 |
| What fraction remains after four half-lives? | 1/16 |
| What fraction remains after n half-lives? | (1/2)^n |
| A sample has a mass of 24.0 g and a volume of 8.0 mL. What formula should you use? | D = m/V |
| A substance has a density of 2.5 g/mL and a volume of 10.0 mL. What formula should you use first? | m = D × V |
| A substance has a mass of 45 g and a density of 3.0 g/mL. What formula should you use? | V = m/D |
| How many moles are in 44 g of CO2? | mol = g/molar mass |
| How many grams are in 2.5 moles of NaCl? | g = mol × molar mass |
| How many particles are in 3.0 moles of helium? | particles = mol × (6.02 × 10^23) |
| How many moles are in 1.204 × 10^24 particles? | mol = particles/(6.02 × 10^23) |
| A solution contains 2.0 moles of solute in 4.0 liters. What formula should you use? | M = mol/L |
| How many moles are in 500 mL of a 2.0 M solution? | mol = M × L |
| A solution has 0.50 mol dissolved in 0.25 L. What formula should you use? | M = mol/L |
| A chemist dilutes 50 mL of a 4.0 M solution to a concentration of 1.0 M. What formula should you use? | M1V1 = M2V2 |
| What volume of a 6.0 M stock solution is needed to make 500 mL of a 2.0 M solution? | M1V1 = M2V2 |
| A solution contains 15 g of solute and 85 g of solvent. What formula should you use first? | mass solution = mass solute + mass solvent |
| A solution contains 15 g of solute and 100 g of solution. What formula should you use? | % mass = mass solute/mass solution × 100 |
| A solution contains 25 mL of ethanol in 200 mL of solution. What formula should you use? | % volume = volume solute/volume solution × 100 |
| A water sample contains 0.002 g solute in 1000 g solution. What formula should you use? | ppm = mass solute/mass solution × 1,000,000 |
| How much heat is absorbed by 50 g of water heated from 20°C to 80°C? | q = mCΔT |
| A sample is heated from 25°C to 75°C. What formula should you use first? | ΔT = Tf - Ti |
| How much energy is required to melt 20 g of ice? | q = mHf |
| How much energy is required to vaporize 10 g of water? | q = mHv |
| A potential energy diagram shows reactants at 300 kJ and products at 150 kJ. What formula should you use? | ΔH = PEproducts - PEreactants |
| What is the pH of a solution with [H+] = 1 × 10^-3 M? | pH = -log[H+] |
| What is the pOH of a solution with [OH-] = 1 × 10^-5 M? | pOH = -log[OH-] |
| A solution has a pH of 3. What formula should you use to find pOH? | pH + pOH = 14 |
| A solution has [H+] = 1 × 10^-6 M. What formula should you use to find [OH-]? | [H+][OH-] = 1 × 10^-14 |
| A solution has [OH-] = 1 × 10^-2 M. What formula should you use to find [H+]? | [H+][OH-] = 1 × 10^-14 |
| 25.0 mL of HCl is neutralized by 30.0 mL of NaOH. What formula should you use? | MaVaia = MbVbib |
| A titration involves H2SO4 and NaOH. What formula should you use? | MaVaia = MbVbib |
| A gas occupies 2.0 L at 300 K and is heated to 600 K. What formula should you use? | P1V1/T1 = P2V2/T2 |
| A gas changes pressure, volume, and temperature. What formula should you use? | P1V1/T1 = P2V2/T2 |
| A gas sample's pressure, volume, temperature, and moles are known except for one variable. What formula should you use? | PV = nRT |
| A gas law problem gives temperature in Celsius. What formula should you use first? | K = °C + 273 |
| The mass number of an atom is 35 and its atomic number is 17. What formula should you use? | neutrons = mass number - atomic number |
| An element has isotopes with different abundances. What formula should you use? | average atomic mass = Σ(isotope mass × decimal abundance) |
| How much of a radioactive sample remains after 4 half-lives? | remaining fraction = (1/2)^n |
| A sample starts with 80 g and undergoes 3 half-lives. What formula should you use first? | remaining fraction = (1/2)^n |
| How much energy is released when 0.001 kg of matter is converted into energy? | E = mc^2 |
| A problem gives ΔH, T, and ΔS and asks whether a reaction is spontaneous. What formula should you use? | ΔG = ΔH - TΔS |
| A solution contains 58.5 g of NaCl dissolved to make 1.0 L of solution. To find molarity, what formulas should you use? | mol = g/molar mass THEN M = mol/L |
| How many particles are present in 36 g of water? | mol = g/molar mass THEN particles = mol × (6.02 × 10^23) |
| What is the percent by mass of a solution containing 20 g solute and 180 g solvent? | mass solution = mass solute + mass solvent THEN % mass = mass solute/mass solution × 100 |
| A titration asks for the concentration of an acid after giving volumes and base concentration. What formula should you use? | MaVaia = MbVbib |
| How much heat is needed to raise the temperature of water and then vaporize it? | q = mCΔT THEN q = mHv |
| How much heat is needed to melt ice and then warm the resulting liquid water? | q = mHf THEN q = mCΔT |
| A gas law problem gives Celsius temperatures and asks for final volume. What formulas should you use? | K = °C + 273 THEN P1V1/T1 = P2V2/T2 |
| A solution's pH is given and you need [OH-]. What formulas should you use? | pH + pOH = 14 THEN pOH = -log[OH-] |
| A solution's [H+] is given and you need pOH. What formulas should you use? | pH = -log[H+] THEN pH + pOH = 14 |
| A sample's mass and density are given and you need the number of particles. What formulas should you use? | V = m/D if needed, then mol = g/molar mass, then particles = mol × (6.02 × 10^23) |
Created by:
markoii