Name_____________________________________________period_____________IB chem
Ch. 1B worksheet
Read chapter 1
1. Consider two people of the same mass standing in a room. One person is standing normally, and the other is
standing on one foot.
a. Does one person exert greater force on the floor than the other? No
b. Does one person exert a greater pressure on the floor than the other? Yes, the person standing on one foot
exerts more pressure because they are standing on a smaller area
2. Convert the following
a. 265 torr to pascals
b. 675 mmHg to atm
c. 5 atm to kPa
4
3.53 x 10 Pa
0.888 atm
500 kPa
3. What is Avogadro’s hypothesis?
Equal volumes of different gases contain equal number of particles at the same temp. and pressure
4. Nitrogen and hydrogen gases react to form ammonia gas, NH3
a. Write a balanced chemical equation
N2 + 3H2  2NH3
b. At a certain temperature and pressure 0.70 dm3 of nitrogen gas reacts with 2.1 dm3 of hydrogen gas. If
all the nitrogen and hydrogen are consumed, what volume of ammonia, at the same temp. and
pressure, will be produced?
1.4 dm3
c. What volume of nitrogen is needed to form 15.0 cm3 of ammonia, NH3.
7.5 cm3
d. What volume of hydrogen is needed when 100.0 cm3 of nitrogen gas reacts?
300 cm3
5. What is STP?
Standard temperature and pressure (0⁰C and 1 atm)
6. What is the molar volume of gas at STP?
22.4 dm3/mol
7. What is RTP?
Room temperature and pressure (25⁰C and 1atm)
8. What is the molar volume of gas at RTP?
24 dm3/mol
9. Calculate the volume occupied by 6.70 g of carbon monoxide at STP.
5.36 dm3
10. Calculate the volume occupied by 11.3 g of nitrogen at RTP.
9.68 dm3
11. How many grams of chlorine are in 34.0 cm3 of gas at STP.
0.108 g
12. a. How many grams of hydrogen gas can be produced by reacting 32.8 g of magnesium according to the
following balanced equation?
Mg (s) + 2 HCl (aq)  MgCl2 (aq) + H2 (g) 2.70 g
b. What volume of hydrogen gas was produced if this reaction was carried out at STP?
30.2 dm3
13. Nitrogen gas can be produced by reacting Na3N with chlorine gas. If the reaction was carried out at STP with
34.8 g of Na3N, what volume of nitrogen gas can be produced?
4.70 dm3
14. Propane reacts with oxygen to form carbon dioxide and water. If 34.4 L of CO2 was produced. What volume
of propane (C3H8) were combusted? Assume the reaction took place at STP.
11.5 dm3
15. A fixed quantity of gas at 23⁰C exhibits a pressure of 748 torr and occupies a volume of 10.3 L. Calculate the
volume the gas will occupy if the temperature is increased to 145 ⁰C
15 dm3
16. A fixed quantity of gas at 21⁰C exhibits a pressure of 748 torr and occupies a volume of 10.3 L. Calculate the
volume the gas will occupy if the temperature is increased to 36 ⁰C and the pressure is decreased to 700 torr.
12 dm3
17. Calculate the following for an ideal gas
a. The volume of gas if 1.57 mol has a pressure of 0.86 atm at a temperature of -12 ⁰C. 39 dm3
b. The temp. of a gas of which 0.0679 mol occupies 164 mL at 693 torr. 26.8 K
c. The pressure, in atm, if 0.0825 mol occupies 255 mL at 115⁰C 10.3 atm
d. The grams of gas, if 5.49L at 35 ⁰C has a pressure of 11.25 kPa. 0.67 g
18. The Hindenburg was a famous hydrogen-filled dirigible that exploded in 1937. If the Hindenburg held 2.0 x
105 m3 of hydrogen gas at 23 ⁰C and 1.0 atm, what mass of hydrogen was present?
1.6 x 107 g
19. Calculate the number of molecules in a deep breath of air whose volume is 2.55 L at body temperature, 37
⁰C, and a pressure of 740 torr
5.9 x 1022 molecules
20. 23.5 g of CO2 gas is at a temperature of 45oC and a pressure of 125 kPa. What is the volume of the container?
11 dm3
21. If 128g of a certain gas in a container with a volume of 21.5 L has a pressure of 132 kPa and a temperature of
45oC, what is the molar mass of the gas? 120 g/mol
22. If 4.0 L of a gas were produced at STP and the mass of the gas was found to be 12.8g, then what is the molar
mass of the gas?
72 g/mol
23. What is a solution? What is a solute? What is a solvent?
A homogeneous mixture; The solute is what is being dissolved and the solvent does the dissolving
24. Label the solute and solvent in each of the following
a. Water vapor in air
b. Carbonated water
c. Hot tea
d. salt water
Solute: water
carbon dioxide
tea
salt
Solvent: air
water
water
water
25. What is the symbol for a solution where the solvent is water? aq
26. What is a saturated solution? The solvent is holding the maximum amount of solute
27. What is the concentration of a solution when 5.0 moles of hydrochloric acid are dissolved in 4.3 dm3 of
solution? 1.2 mol dm-3
28. What is the concentration of a solution when 45 g of sodium hydroxide are dissolved in 250 cm3 of solution?
4.5 mol dm-3
29. A solution of calcium hydroxide has a concentration of 7.5 g dm-3. What is the concentration in mol dm-3?
0.10 mol dm-3
30. A solution of potassium chloride has a concentration of 5.4 mol dm-3. What is the concentration in g dm-3?
4.0 x 102 g dm-3
31. How many grams of barium nitrate are needed to make 250 cm3 of a 1.75 mol dm-3 solution?
87 g
32. How many moles of sodium hydroxide are contained in 6.50 dm3 of a 2.20 mol dm-3 solution?
14.3 mol
33. A solution is made by dissolving 17.1 g of sucrose, C12H22O11 in 275 cm3 of water.
a. What is the solute? sucrose
b. What is the solvent? water
c. What is the concentration? 0.182 mol dm-3
34. What volume of hydrochloric acid with a concentration of 1.40 mol dm-3 would have to be added to 15.0 cm3
of 0.800 mol dm-3 sodium hydroxide solution to produce a neutral solution?
8.57 cm3
35. 25.00 cm3 of 0.100 mol dm-3 sodium hydrogencarbonate solution was titrated with sulfuric acid:
2NaHCO3 (aq) + H2SO4 (aq)  Na2SO4 (aq) + 2H2O(l) + 2CO2 (g)
15.2 cm3 of the acid was needed to neutralize the solution.
a. calculate the concentration of the sulfuric acid.
0.329 mol dm-3
b. calculate the volume of carbon dioxide, measured at STP produced during the titration
0.056 dm3
36. Round the following numbers so that they contain 3 significant figures.
a) 173,792
b) 0.0025021
c) 0.0003192
d) 30
173,000
0.00250
0.000319
30.0
37. Define the term isotope.
Atoms with different masses (same number of protons but different number of neutrons)
38. Does an electron need to absorb energy or give off energy to go from the 2nd to the 1st energy level?
Give off
39. Given the following compounds, determine the charge on the unknown ion “X”.
a) X2S
b) MgX
c) X3P2
+1
-2
+2
40. Balance the following reaction: _____ Al2S3 + __3___ Cu  ___3__ CuS + __2___ Al
41. Find the formula mass for each of the following (include units):
a) magnesium phosphide 134.9 amu
b) sodium sulfate 142.1 amu
42. In a bag full of pennies, you may have 2.15 moles of copper. How many grams do you have? 0.0339 g
43. Determine the name of the group each belong to
a. Potassium
b. chlorine
c. neon
d. magnesium
e. gold
Alkali metals
halogens
noble gas
alkaline earth metal transition metal
44. How many protons, neutrons, and electrons are in the following
65
Zn2+
b. 40Ar
c. 14N3d. 23Na+
30, 35, 28
18, 22, 18
7,7,10
11, 12,10
45. Which member of the following pairs of substances would you expect to have a higher boiling point?
a. N2 or O2
b. NaCl or CH3Cl
c. CH3Cl or CH4