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Chemistry Semester 2 Final Exam
Terms in this set (25)
Which of the following compounds contains the lead(II) ion?
Which of the following shows both the correct formula and correct name of an acid?
a. HClO₂, chloric acid
b. HNO₂, hydronitrous
c. H₃PO₄, phosphoric acid
d. HI, iodic acid
How many moles of tunsten atoms are in 4.8 x 10²⁵ atoms of tungsten?
a. 8.0 x 10² moles
b. 8.0 x 10¹ moles
c. 1.3 x 10⁻¹ moles
d. 1.3 x 10⁻² moles
What is molar mass of (NH₄)₂CO₃?
How many moles of CaBr₂ are in 5.0 grams of CaBr₂?
a. 2.5 x 10⁻² mol
b. 4.2 x 10⁻² mol
c. 4.0 x 10¹ mol
d. 1.0 x 10³ mol
What is the volume, in liters, of 0.500 mol of C₃H₈ gas at STP?
a. 0.0335 L
b. 11.2 L
c. 16.8 L
d. 22.4 L
What is the percent by mass of carbon in acetone, C₃H₆O?
What are the missing coefficients for the skeleton equation below when it is correctly balanced?
Cr(s) + Fe(NO₃)₂(aq) → Fe(s) + Cr(NO₃)₃(aq)
a. 4, 6, 6, 2
b. 2, 3, 2, 3
c. 2, 3, 3, 2
d. 1, 3, 3, 1
Which of the following is a balanced equation representing the decomposition of lead(IV) oxide?
a. PbO₂→Pb + 2O
b. PbO₂→Pb + O₂
c. Pb₂O→2Pb + O
d. PbO→Pb + O₂
The equation Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g) is an example of which type of reaction?
a. combination reaction
b. single-replacement reaction
c. decomposition reaction
d. double-replacement reaction
When iron rusts in air, iron (III) oxide is produced. How many moles of oxygen react with 2.4 mol of iron in the rusting reaction?
4Fe(s) + 3O₂(g) → 2Fe2O₃(s)
a. 1.2 mol
b. 1.8 mol
c. 2.4 mol
d. 3.2 mol
At STP, how many liters of oxygen are required to react completely with 3.6 liters of hydrogen to form water?
2H₂(g) O₂(g) → 2H₂O(g)
a. 1.8 L
b. 3.6 L
c. 2.0 L
d. 2.4 L
Mercury can be obtained by reacting mercury(II) sulfide with calcium oxide. How many grams of calcium oxide are needed to produce 36.0g of Hg?
4HgS(s) + 4CaO(s) →4Hg(l) + 3CaS(s) + CaSO₄
When two substances react to form products, the reactant which is used up is called the ________.
a. determining reagent
b. limiting reagent
c. excess reagent
d. catalytic reagent
Standard conditions when working with gases are defined as ________.
a. 0°K and 101.3 kPa
b. 0°K and 1 kPa
c. 0°C and 101.3 kPa
d. 0°C and 1 kPa
Which of these changes would NOT cause an increase in the pressure of a contained gas?
a. the volume of the container is increased
b. more of the gas is added to the container
c. the temperature is increased
d. the average kinetic energy of the gas increased
Charles's law states that ________.
a. the pressure of a gas is inversely proportional to its temperature in kelvins
b. the volume of a gas is directly proportional to its temperature in kelvins
c. the pressure of a gas is directly proportional to its temperature in kelvins
d. the volume of a gas is inversely proportional to its temperature in kelvins
How many significant figures are in the measurement 40,500 mg?
Express the sum of 7.68m and 5.0m using the correct number of significant digits.
a. 12.68 m
b. 12.7 m
c. 13 m
d. 10 m
Express the product of 4.0 x 10⁻² m and 8.1 x 10² m using the correct number of significant digits.
a. 3 x 10¹
b. 3.0 x 10¹
c. 3.2 x 10¹
d. 3.24 x 10¹
What is the density of an object having a mass of 8.0 g and volume of 25 cm³?
a. 0.32 g/cm³
b. 2.0 g/cm³
c. 3.1 g/cm³
d. 200 g/cm³
What element in the second period has the largest atomic radius?
What is the element with the highest electronegativity value?
What element is represented by the following noble gas notation: [Ar]4s²
a. Sulfur (S)
b. Magnesium (Mg)
c. Calcium (Ca)
d. Argon (Ar)
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