| Chapter 1 Chemistry 1201/1202 |
|
|
| Give the chemical symbol or name for the following elements, as appropriate: (a) sulfur, (b) magnesium, (c) potassium, (d) chlorine, (e) copper, (f) F, (g) Ni, (h) Na, (i) Al, (j)Si |
|
|
| Make the following conversions: (a) 62 degree Farenheit to Celsius, (b) 216.7 degree Celsius (c) 233 degrees Celsius to Kelvin, (d) 315 K to degrees Farenheit (e) 2500 degrees Farenheit to Kelvin. |
|
|
Round each of the following numbers to four significant figures, and express the result in standard exponential notation: (a) 102.
Don’t waste time
Get Your Custom Essay on
“EDCI Assignment 3”
Get High-quality Paper
helping students since 2016
53070, (b) 656,980, (c)0.008543210, (d) 0.000257870, (e) -0.0357202 |
|
|
| By using estimation techniques, arrange these items in order from shortest to longest: a 57-cm length of string, a 14-in. long shoe, and a 1.1-m length of pipe. |
|
|
| A 32.65-g. sample of a solid is placed in a flask. Toluene, in which the solid is insoluble, is added to the flask so that the total volume of solid and liquid together is 50.00 mL. The solid and toluene together weight 58.58 g. The density of toluene at the temperature of the experiment is 0. 864 g/ mL. What is the density of the solid? |
|
|
| Suppose you are given a sample of a homogeneous liquid. What would you do to determine whether it is a solution or a pure substance? |
|
|
| Chapter 2 Chemistry 1201/1202 |
|
|
| Four of the boxes in the following periodic table are colored. Which of these are metals and which are nonmetals? Which one is an alkaline earth metal? Which is a noble gas? [Image on back] |
|
|
| Fill in the gaps in the following table, assuming each column represents a neutral atom:[Image on back] |
|
|
| How many hydrogen atoms are in each of the following: (a) C2 H5 OH (b) Ca (CH3 COO)2 , (c) (NH4 )3 PO4 ? |
|
|
| Write the chemical formulas for the follwing compounds: (a) aluminum hydroxide, (b) potassium sulfate, (c) copper (I) oxide, (d) zinc nitrate, (e) mercury (II) bromide, (f) iron (III) carbonate, (g) sodium hypobromite. |
|
|
| The element oxygen has three naturally occuring isotopes, with 8,9,10 neutrons in the nucleus, resepctively. (a) Write the full chemical symbols for these three isotopes. (b) Describe the similarities and differences between the three kinds of atoms of oxygen. |
|
|
| From the molecular structures shown here, identify the one that corresponds to each of the following species: (a) Chlorine gas; (b) propane, (c) nitrate ion; (d) sulfur trioxide; (e) methyl chloride, CH3 Cl. [Image on back] |
|
|
| Chapter 3 Chemistry 1201/1202 |
|
|
|
(a) What is the difference between adding a subscript 2 to the end of the formula CO to give CO2 and adding a coefficent in front of the formula to give 2 CO? (b) Is the following chemical equation, as written, consistent with the law of conservation of mass?
3Mg(OH)2 (s) + 2 H3 PO4 (aq) ——-> Mg3 (PO4)2 (s) + 6 H2 O(l)
|
|
|
|
Balance the following equations, and indicate whether they are combination, decomposition, or combustion reactions:
(a) Al (s) + Cl2 (g) ——> AlCl3 (s)
(b) C2 H4 (g) + O2 (g) —–> CO(g) + HO(g)
(c) Li(s) + N2 (g) —–> Li3N(s)
(d) PbCO3 (s)—–> PbO(s) + CO2 (g)
(e) C7H8O2(l) + O2(g) ——> CO2 (g) + H2O (g)
|
|
|
| Determine the formula weights of each of the following compounds: (a) nitric acid, HNO3 ; (b) KMnO4; (c) Ca3 (PO4 )2 ; (d) quartz, SiO2; (e) gallium sulfide, (f) chromium (III) sulfate, (g) phosphorus trichloride. |
|
|
| The molecular formula of allicin, the compound responsible for the characteristic smell of garlic, is C6 H10 OS2 . (a) What is the molar mass of allicin? (b) How many moles of allicin are present in 5.00 mg of this substance? (c) How many molecules of allicin are in 5.00mg of this substance? (d) How many S atoms are present in 5.00 mg of allicin? |
|
|
| Give the empirical ormula of each of the following compounds if a sample contains (a.) 0.0130 mol C, 0.0390 mol H, and 0.0065 mol O; (b) 11.66 g iron and 5.01 g oxygen; (c) 40.0% C, 6.7% H, and 53.3% O by mass. |
|
|
|
Hydrofluoric acid, HF (aq), cannot be stored in glass bottles because compounds called silicates in the glass are attacked by the HF (aq). Sodium silicate (Na2SiO3), for example, reacts as follows:
Na2SiO3 (s) + 8 HF (aq) —–> H2 SiF6 (aq) + 2 NaF (aq) + 3 H2 O (l)
(a) How many moles of HF are needed to react with 0.300 of Na2SiO3 ?
(b) How many grams of NaF form when 0.500 mol of HF reacts with excess Na2SiO3 ?
(c) How many grams of Na2SiO3 can react with 0.800 g of HF ?
|
|
|
| A manufacturer of bicycles has 4815 wheels, 2305 frames, and 2255 handlebars. (a) How many bicycles can be manufactured using these parts? (b) How many parts of each kind are left over? (c) Which part limits the production of bicycles ? |
|
|
| Chapter 4 Chemistry 1201/1202 |
|
|
| We have learned in this chapter that many ionic solids dissolve in water as strong electrolytes, that is , as separated ions in solution. What properties water faciliate this process? |
|
|
| Will precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction. (a) Na2CO3 and AgNO3, and (b) NaNO3 and NiSO4 (c) FeSO4 and Pb (NO3 )2. |
|
|
| HCl, HBr, and HI are strong acids, yet HF is a weak acid. What does this mean in terms of the extent to wshich theses substances are ionized in solution? |
|
|
| Which circled region of the periodic table shown here contains the most readily oxidized elemnts? Which contains the least readily oxidized? [Image on back] |
|
|
| The average adult human male has a total blood volume of 5.0 L. If the concentration of sodium ion in this average individual is 0.135 M, what is the mass of sodium ion circulating in the blood? |
|
|
| What mass of KCl is needed to precipitate the sivler ions from 15.0 mL of 0.200 M AgNO3 solution? |
|
|
| Chapter 5 Chemistry 1201/1202 |
|
|
| Consider the accompanying energy diagram. (a) Does this diagram represent an increase or decrease in the internal energy of the system? (b) What sign is given to delta E(energy) for this process? (c) If there is no work associated with the process, is it exothermic or endothermic?[Image on back] |
|
|
| (a) Calculate the kinetic energy in joules of a 45-g golf ball moving at 61 m/s. (b) Convert this energy to calories. (c) What happens to this energy when the ball lands in a sand trap? |
|
|
| Calculate delta E (energy), and determine whether the process is endothermic or exothermic for the follwing cases: (a) A system absorbs 105 kJ of heat from its surroundings while doing 29 kJ of work on the surroundings; (b) q= 1.50 kJ and w = – 657 J; (c) the system releases 57.5 kJ of heat while doing 22.5 kJ of work on the surroundings. |
|
|
| You are given delta H (enthalpy) for a process that occurs at constant pressure. What additional information do you need to determine delta E (energy) for the process? |
|
|
| (a) What is the specific heat of liquid water? (b) What is the molar heat capacity of liquid water? (c) What is the heat capacity of 185 g of liquid water? (d) How many kJ of heat are needed to raise the temperature of 10.00 kg of liquid water from 24.6 degrees Celsius to 46.2 degrees Celsius? |
|
|
|
Calculate the enthalpy change for the reaction
P4O6 (s) + 2 O2 (g) —–> P4O10(s)
given the following enthalpies of reaction:
P4(s) + 3O2(s)———-> 2H2O(g) delta H = -483.6 kJ
P4(s) + 5O2(g)———-> 2 O3 (g) delta H = +284.6 kJ
|
|
|
| (a) What is meant by the term standard conditions, with reference to enthalpy changes? (b) What is meant by the term enthalpy of formation? (c) What is meant by the term standard enthalpy of formation? |
|
|
