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Chem Final Exam
| Question | Answer |
|---|---|
| How should the total weight; 64.382, be reported as? a. 64.4 g b. 64.382 g c. 64.38 g d. 64 g | 64.38 g |
| Which of the following has four significant figures? a. 0.0075 b. 0.0750 c. 7.500 d. 0.0705 | 7.500 |
| Add 8.487 g, 0.31 g, and 0.0042 g. The answer to the correct number of sig figs after the decimal point is: a. 8.8012 g b. 8.801 g c. 8.80 g d. 8.8 g | 8.80 g |
| Express the following in standard decimal form: 9.300 x 10^-7 M | 0.00000093 |
| What is an exact number? | a number that is considered to have an infinite number of sig figs |
| How many digits are needed for measured numbers in a lab? | 2-3 digits |
| Are non-zero digits always counted? | Always |
| Are beginning zeros always counted? | Never |
| Are between zeros always counted? | Always |
| Are ending zeros always counted? | Only when a decimal point is showing |
| An ibuprofen suspension for infants contains 100mg/5.0 mL suspension. The recommended dose is 10mg/Kg body weight. How many mL of this suspension should be given to an infant weighing 18 lbs? | 4.08 mL |
| A candy bar contains 225 Cal of nutritional energy. How many joules does it contain? | 971,000 Joules |
| Compound | Composed of 2 or more separate elements held together by chemical bonds |
| Pure Substance | Single kind of matter that cannot be separated into other kinds of matter |
| Mixtures | Substances made by mixing other substances together |
| Homogenius mixture | Mixture in which the composition is uniform throughout the mixture |
| Heterogenius mixture | Mixture in which the composition is not uniform throughout the mixture |
| Gallium is a solid metal at room temperature but melts at 29.9 C. How much heat must 2.5 g of gallium absorb from your hand to raise the temperature of the gallium from 25.0 C to 29.9 C? the specific heat capacity of gallium is 0.327 J/g C. | 4.0 Joules |
| How many protons are in the element, Carbon? | 6, same number as atomic number |
| Cation | Ions that are positively charged |
| Anion | Ions that are negatively charged |
| Name the 7 diatomic elements found naturally. | O2, H2, I2, N2, F2, Cl2, Br2 |
| If we decompose 17.0 g of ammonia (NH3), we get 14.0 g of nitrogen and 3.0 g of hydrogen. What is the mass ratio of nitrogen to hydrogen? | 4:7 |
| Write the empirical formula for B2H6 | BH3 |
| Ionic Compounds | Metal + nonmetal Metal+ semimetal |
| Molecular Compounds | Nonmetals Semimetal+ nonmetals |
| 4.8 mol of copper is how many atoms? | 2.9 x 10^24 atoms |
| 1.1 x 10^22 silver atoms is how many moles? | 0.018 moles |
| Calculate the mass of sulfur in 2.78 mol of sulfur | 89.2 grams |
| Calculate the moles of sulfur in 57.5 g of sulfur | 1.79 moles |
| Calculate the number of atoms in a 48.3 g sample of zinc | 4.4 x 10^33 atoms |
| Calculate the number of atoms in an aluminum can that has a mass of 16.2 g | 3.6 x 10^33 atoms |
| Convert between grams and moles using molar mass: 72.5 g of CCl4 | 0.47 mol CCl4 |
| Convert between grams and moles using molar mass: 25.2 Kg of C2H2 | 967.9 mol C2H2 |
| Convert between grams and moles using molar mass: 15.7 mol of HNO3 | 989 g HNO3 |
| How many molecules are in 6.5 g of H2O? | 2.17 x 10^23 molecules |
| Determine the number of moles of O in 1.7 mol of CaCO3. | 5.1 O moles |
| Calculate mass (in grams) of sodium in 8.5 g of each sodium containing food additive; NaCl | 3.34 g |
| Calculate the mass percent composition of the underlined element in each of the follow compounds; C in CH4 | 74.7% |
| Calculate the empirical formula for nicotine C: 74.03%, H:8.70%, N 17.27% | C2H7N1 |
| What are the 5 indicators of a chem reaction? | 1. Color change 2. Formation of a precipitate 3. Formation of a gas 4. Odor change 5. Temperature change |
| Write a balanced chemical equation: Solid magnesium reacts with aqueous copper (I) nitrate to form aqueous magnesium nitrate and solid copper | 2CuNO3(aq) + Mg (s)=Mg(NO3)2 (aq) + 2Cu (s) |
| Is Mg (s) + O2 (g) =2MgO (s) a redox reaction? | Yes, because it is a combination reaction |
| Combustion reactions produce CO2 and? | Water |
| Combination | A+B=AB |
| Decomposition | AB=A + B |
| Single displacement | A+BC= AC+B |
| Double displacement | AB+CD=AD+CB |
| Precipitation and Acid-base reactions are classified as what type of reaction? | Double displacement |
| How many moles of NaCl can result from the complete reaction of 3.4 moles of Cl2? | 6.8 mol Cl2 |
| How many grams of water result from the reaction of 12.5 g of O2? | 14.1 g H2O |
| What is percent yield? | Actual yield / Theoretical yield x 100 |
| What is the maximum number of electrons in the "d" sublevel? | 10 |
| Order the following elements in order of decreasing atomic size: Mg, Ca, and P | Ca, Mg, P |
| Which of the following elements has the highest ionization energy? a. Sn b. S c. Si d. F | F, increases as you move right |
| Electronegativity | Electrical property that describes the tendency of an atom or a functional group to attract electrons toward itself |
| Arrange the following elements in order of increasing electronegativity | Na, Al, P, N |
| What is the pressure in a 15.0 L cylinder filled with 32.7 g of O2 gas at a temp of 302K? | 1.69 atm |
| You measure the mass of a gas to be 0.311 g at 296 K, 0.217 L and 0.789 atm. What is the molar mass of this gas? | 0.00704 mol |
| Calculate the amount of water in g that can be vaporized at its boiling point with 155 kJ of heat, 40.7 kJ/mol | 68.6 g H2O |
| Use the ideal gas law to show that the molar volume of gas at STP is 22.4 L. | 22.4 L |
| A sample of H2 gas is mixed with H2O vapor. The mixture has a total pressure of 755 torr, and the H2O vapor has a partial pressure of 24 torr. What is the partial pressure of the H2 gas? | 731 PH2 |
| Calculate the amount of ice in g that, upon melting at 0 C, absorbs 237 kJ of heat, 6.02 kJ/mol | 709 g |
| Dispersion forces | a temporary attractive force that results when electrons in 2 adjacent atoms occupy positions that make atoms force temporary dipoles |
| Dipole-Dipole | Are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule. |
| Hydrogen bonding | Attraction between 2 atoms that already participate in other chemical bonds |
| Ion-Dipole forces | An attractive force that results from the electrostatic attraction between and ion and a neutral molecule that has a dipole, mostly found in solutions |
| Surface tension | The tension of the surface film of a liquid caused by the attraction of the particles in the surface layer by the bulk of the liquid, which tends to minimize surface area |
| Melting point and boiling point both ______ with greater intermolecular forces | Increase |
| _______ also increase melting and boiling points | Larger surface areas |
| Which halogen has the highest boiling point? Cl2, I2, or Br2 | Iodine, higher boiling point and higher mass |
| n-pentane (C5H12) has a boiling point of 36.1 C and neopentane has a boiling point of 9.5 C, why? | n-pentane, because it has more surface area |
| Which has a higher boiling point, HF or HCl? | HF, strong dipole forces and is the most electronegative |
| Example of a molecular solid: | Salt, Sodium Chloride |
| Example of an ionic solid: | Potassium Bromide |
| Example of an atomic solid: | Fe, pure iron |
| Solution | A homogenous mixture of one or more solutes dissolved in a solvent |
| Solute | The substance that dissolves in a solvent to produce a homogeneous mixture |
| Solvent | Substance in which a solute dissolves to produce a homogeneous mixture |
| Saturated Solution | A solution with solute that dissolves until it is unable to dissolve anymore, leaving the undissolved substances at the bottom. |
| Unsaturated Solution | A solution (with less solute than the saturated solution) that completely dissolves, leaving no remaining substances. |
| Supersaturated Solution | A solution that contains more dissolved solute than required for preparing a saturated solution and can be prepared by heating a saturated solution, adding more solute, and then cooling it gently. |
| What is the difference between electrolyte vs a non-electrolyte solution? | Electrolytes conduct electric current when in solution or melted, nonelectrolytes do no conduct electric current when in solution or melted |
| Find the mass percent of a solution containing 19 g of solute and 158 g of solvent. | 11% |
| How much KCl is in 0.337 L of a 5.80% mass percent KCl solution? density of solution is 1.05 g/mL | 20.5 g KCl |
| Calculate the molarity of a KCl solution containing 0.22 mol of KCl in 0.455 L of solution | 0.48 mol KCl |
| How much KCl in grams is contained in 0.488 L of 1.25 M KCl solution? | 45.4 g |
| What is the concentration of Cl- ions in a 1.5 M CaCl2? | 3.0 M Cl- |
| How much of an 8.0 M HCl solution should you use to make 0.400 L of a 2.7 M HCl solution? | 0.135 L |
| Calcuate the molality of a solution, if 91.3 g of sugar (C6H12O6) is dissolved in 125 g of H2O | 4.06 m |
| Calculate the freezing point depression of a 1.9 m salt water solution? Kf=1.86 C kg/mol | -3.4 C |
| Calculate the boiling point elevation of a 1.7 m salt water solution? Kf=0.512 C kg/mol | 100.87 C |
| Characteristics of acids: | Conduct electricity, change blue litmus to red, has a sour taste, react with bases to neutralize their properties |
| Characteristics of bases: | Conduct electricity, change red litmus to blue, have a slippery feeling, react with acids to neutralize their properties |
| Brosnted Lowry definition of acids: | Can donate a hydrogen ion |
| Brosnted Lowry definition of bases: | Compound that can accept a hydrogen ion |
| What is the conjugate acid for NH3? | NH4+ |
| In the following reaction: HCO3- (aq)+H2O (aq)=H2CO3 (aq)+OH- (aq) which is the acid and its conjugate base? | H2O is an acid and OH- is its conjugate base |
| What is neutralization? | Chemical reaction in which acid and a base react quantitively with each other |
| Give an example of an acid reacting with a metal or metal oxide: | A small amount of copper oxide is added to sulphuric acid, the color of the solution becomes blue and the copper oxide dissolves, indicating the formation of Copper II sulphate |
| A 25.0 mL sample of 0.105 M HCl was titrated with 31.5 mL of NaOH. What is the concentration of the NaOH? | 0.0833 M |
| A 35.0 mL sample of 0.225 M HBr was titrated with 42.3 ML of KOH. What is the concentration of the KOH? | 0.186 M |
| List the strong acids: | HCl, HNO3, H2SO4, HBr, HI, HClO4 |
| What is the concentration of H+ in 2.0 M acetic acid? | <2.0 M |
| What is the concentration of H+ in 0.50 M hydrochloric acid? | 0.50 M |
| List strong bases: | LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2 |
| List weak bases: | NH3, C5H5N, CH3NH2, C2H5NH3, HCO3- |
| HF is an example of an ____ acid. | weak |
| Which solution has the highest concentration of hydroxide ions? a. pH=3.21 b. pH=12.49 c. pH=7.00 d. PH=10.12 | pH=12.49, basic substances are above 7 |
| What is a buffer solution? | The solutions which resist the change in pH on dilution or with the addition of small amounts of acid or alkali |
| Which combination will be a buffer solution? a. HCl and Cl- b. HNO3 and NaNO3 c. HC2H3O2 and NaC2H3O2 d. NaBr and NaOH | HC2H3O2 and NaC2H3O2 |
| What increases the reaction rate for chem equilibrium? | An increase in concentration of reactants |
| In an exothermic reaction, it shifts to the _____. | Left |
| In an endothermic reaction, it shifts to the _____. | Right |
| Why does the rate of the reaction decrease over time? | A decrease in concentration of reactions results in fewer successful collisions |
| The effect of a catalyst is to: | Lower the activation energy of a reaction by making it easier for reactants to get over energy hump |
| Which equilibrium constant represents a reaction that favors the formation of the products to the greatest extend? a. Keq=100 b. Keq=1.0 x 10^8 c. 1.0 x 10^-3 d. Keq= 1.0 x 10^-18 | Keq=1.0 x 10^8, choose highest number |
| For chem equilibrium , as the pressure increases, the volume _______ | decreases |
| Which of the following is true of a system for which Keq<<1? | The equilibrium favors the reverse reaction |
| If the [N2]=0.110 M and [H2]=0.0935 M, then what does [NH3] equal? | 0.117 M |
| For the reaction Ag2S (s)=2Ag+ (aq) + S^2- (aq), what happens to the equilibrium position if aqueous ammonium sulfide is added? | Shifts to the left |
| Consider the reaction: 2N2O (g)= O2 (g) + 2N2 (g). Which of the following will cause a shift in the equilibrium to the right? a. add more N2O b. Remove O2 c. Remove N2 | All of 1,2, and 3 |
| For the reaction 2N2O (g)= O2 (g) + 2N2 (g), what happens to the equilibrium postion if the pressure increases? | Shifts to the left |
| For the reaction 2N2O (g)= O2 (g) + 2N2 (g), what happens to the equilibrium positions if the volume decreases? | Shifts to the left |
| What happens to the equilibrium position of an exothermic position when you add heat? | Shifts to the left |
| Which compound is most soluble in water based on its Ksp value? a. CuS, Ksp= 1.27 x 10^-36 b. PbS, Ksp= 9.04 x 10^-29 c. AgCl, Ksp= 1.77 x 10^-10 d. AgI, Ksp= 8.51 x 10^-17 | AgCl, Ksp= 1.77 x 10^-10 |
| What is the [Cu2+] at equilibrium, given CuS, Ksp= 1.27 x 10^-36 a. 1.27 x 10^-36 M b. 6.35 x 10^-37 M c. 1.13 x 10^-18 M d. 1.61 x 10^-72 M | 1.13 x 10^-18 |
| Which of the following atoms has the smallest radius? a. Li b. Ne c. B d. O | Ne |
| Which compound in liquid form will have the highest boiling point? a. non polar CH4 b. non polar CH3CH3 c. polar CH3C(O)CH3 d. polar CH3CH2OH | polar CH3CH2OH |
| How many low dose 85.0 mg aspirin tablets can be made from 13.0 g of aspirin> a. 15.2 tablets b. 15 tablets c. 6.5 tablets d. 152 tablets | 152 |
| How many neutrons are present in C-13? | 7 |
Created by:
Sydboyer15