Answer each of the following question according to the directions. For the drag and drop questions, answer choices may be reused in the same question.
Question 1
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Question 2
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Question 3
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Question 4
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Question 5
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Question 6
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Question 7
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Question 8
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Other Answer Choices:
233.99 g
9 mol
Question 9
9.
Hydrazine, N2H4, and dinitrogen tetroxide, N2O4, react to form gaseous nitrogen and water. Which of these represents a properly balanced equation for this reaction?
To balance an equation ______________ must be placed in front of the compound(s) and or element(s).
subscripts
species
coefficients
reactants
Identify the compound with covalent bonds.
NaCl
CH4
Mg
Ne
Which of the following contains BOTH ionic and covalent bonds?
CaSO4
COS
SF6
CaI2
What is the charge on the Cr ions in Cr2O3?
2-
3+
2+
1+
Calculate the molar mass of Al(C2H3O2)3.
86.03 g/mol
56.00 g/mol
139.99 g/mol
204.13 g/mol
How many moles of N2O4 are in 76.3 g N2O4? The molar mass of N2O4 is 92.02 g/mol.
1.21 moles
0.829 moles
7.02 x 103 moles
1.42 x 10-4 moles
How many atoms of oxygen are contained in 47.6 g of Al2(CO3)3? The molar mass of Al2(CO3)3 is 233.99 g/mol.
47.6 g x (1mol/_____________ ) x (__________ /1mol) x(______________________ ) = ______________________
6.02 x 1023 atoms
1.10 x 1024 atoms
When methane (CH4) gas is burned in the presence of oxygen, the following chemical reaction occurs.
CH4 + 2O2 → CO2 + 2H2O
If 1 mole of methane reacts with 2 moles of oxygen, then
6.02 x 1023 molecules of CO2 and 1.2 x 1024 molecules of H2O are produced
1.2 x 1024 molecules of CO2 and 1.2 x 1024 molecules of H2O are produced
6.02 x 1023 molecules of CO2 and 6.02 x 1023 molecules of H2O are produced
1.2 x 1024 molecules of CO2 and 6.02 x 1023molecules of H2O are produced
A balanced chemical equation reflects the idea that the mass of the products
is less than the mass of the reactants
is not related to the mass of the reactants
equals the mass of the reactants
is greater than the mass of the reactants
A student heated a 10 g sample of a compound in an open container. A chemical reaction occurred. The mass of the sample was measured again and found to be less than before. Which of the following explains the change in mass of the sample?
Some of the lighter atoms were converted to energy.
One of the reaction products was a gas.
The reaction gave off more heat than was added.
The heat caused the compound to become less dense.
The chemical equation below represents sulfur trioxide (SO3) in the atmosphere mixing with rainwater to form sulfuric acid (H2SO4), which is a major component of acid rain.
SO3(g) + H2O(l) --> H2SO4(l)
How much H2SO4 is produced when 128.0 g of SO3 mixes with rainwater?
SO3: (1 x 32) + (3 x 16) =_________H2SO4: (2 x 1) + (1 x 32) + (4 x 16) = _________
Solution:
(__________ / _________)x _________ = __________
The equation below represents a balanced chemical reaction:
2Mg(s) + O2(g) --> 2MgO(s)
How many moles of MgO are produced when 7.2 moles of O2 react with excess Mg?
3.6 moles
14 moles
29 moles
22 moles
What type of force holds ions together in salts such as CaF2?
gravitational
nuclear
electrostatic
magnetic
Which of the following pairs of atoms is unlikely to form a compound?
potassium (K) and iodine (I)
iron (Fe) and sulfur (S)
neon (Ne) and argon (Ar)
calcium (Ca) and chlorine (Cl)
Use the diagram to answer the following question.
How many bonds are made by each carbon atom in the molecule shown above?
three
four
two
one
Two elements in a molecule have the same electronegativity values. Which of the following most likely holds the elements together and why?
an intermolecular force, because the elements do not form a chemical bond
an ionic bond, because electrons transfer from one element to the other
a nonpolar covalent bond, because the elements share electrons equally
a polar covalent bond, because the elements do not share electrons equally
Which of the following are most directly involved in chemical bonding?
protons
neutrons
alpha particles
valence electrons
Ionic Bond
Covalent Bond
Metallic Bond
Higher melting point
Lower melting point
Brittle and hard
Exists as solid, liquid, and gas at STP
Malleable and lustrous
Conductive as a solid
Poor conductor
Lattice made of positive and negative ions
Lattice of positive ions surrounded by sea of electrons
Shared electrons between two or more atoms
For the reactions below, select the correct reaction type and drag it onto the equation.
Synthesis
Single Replacement
Decomposition
Combustion
Double Replacement
C2H4 + 3O2 --> 2CO2 + 2H2O
Place the items in order to show how to solve a grams to mole stoichiometry problem.