Chemistry 101 Final Ivy Tech Questions With Complete
Solution | 2024
Diatomic O2 can react with the element magnesium to form magnesium oxide (MgO). The
balanced chemical equation is:
O2 + Mg ⟶ 2 MgO
If 4 moles of magnesium totally reacted with more than enough O2, how many moles of
MgO would be expected to form?
A. 8 Moles
B. 2 Moles
C. 4 Moles
D. 1 Mole
E. Not Enough Info - -C
Which of the following is TRUE?
,A. Stoichiometry allows prediction of how much of the reactants are necessary to form a
given amount of product.
B. All of the above are true.
C. Stoichiometry allows prediction of the amount of products that form in a chemical
reaction based on the amounts of reactants.
D. Stoichiometry shows the numerical relationship between chemical quantities in a
balanced chemical equation. - -B
Diatomic N2 can react with diatomic H2 to form ammonia (NH3). The balanced chemical
equation is:
N2 + 3 H2 ⟶ 2 NH3
If 6 moles of H2 totally reacted with more than enough N2, how many moles of ammonia
would be expected to form?
,A. 4 Moles
B. 6 Moles
C. 3 Moles
D. 2 Moles
E. Not enough info - -A
How many grams of the excess reactant remain assuming the reaction goes to completion
and that you start with 15.5 g of Na2S and 12.1 g of CuSO4?
Reaction: Na2S+ CuSO4 ⟶ Na2SO4 + CuS
A. 0.05
B. 9.58
C. 5.92
D. 15.45 - -B
Consider the following reaction: 2 Mg + O2 ⟶ 2 MgO Δ Hrxn = -1203 kJ. Calculate the
amount of heat (in kJ) associated with complete reaction of 4 moles of Mg.
A. -1203 kJ
, B. -601.5 kJ
C. -4812 kJ
D. None of the above
E. -2406 kJ - -E
Hydrochloric acid reacts with barium hydroxide according to the equation:
2 HCl (aq) + Ba(OH)2 (aq) ⟶ BaCl2 (aq) + 2 H2O ( l) Δ H= -118 kK
Calculate the heat (in kJ) associated with the complete reaction of 18.2 grams of HCl (aq).
A. -58.9
B. -29.5
C. None of above
D. -236
E. +58.9 - -B
How many grams of NO2 are theoretically produced if we start with 1.2 moles of S and 9.90
moles of HNO3?
Solution | 2024
Diatomic O2 can react with the element magnesium to form magnesium oxide (MgO). The
balanced chemical equation is:
O2 + Mg ⟶ 2 MgO
If 4 moles of magnesium totally reacted with more than enough O2, how many moles of
MgO would be expected to form?
A. 8 Moles
B. 2 Moles
C. 4 Moles
D. 1 Mole
E. Not Enough Info - -C
Which of the following is TRUE?
,A. Stoichiometry allows prediction of how much of the reactants are necessary to form a
given amount of product.
B. All of the above are true.
C. Stoichiometry allows prediction of the amount of products that form in a chemical
reaction based on the amounts of reactants.
D. Stoichiometry shows the numerical relationship between chemical quantities in a
balanced chemical equation. - -B
Diatomic N2 can react with diatomic H2 to form ammonia (NH3). The balanced chemical
equation is:
N2 + 3 H2 ⟶ 2 NH3
If 6 moles of H2 totally reacted with more than enough N2, how many moles of ammonia
would be expected to form?
,A. 4 Moles
B. 6 Moles
C. 3 Moles
D. 2 Moles
E. Not enough info - -A
How many grams of the excess reactant remain assuming the reaction goes to completion
and that you start with 15.5 g of Na2S and 12.1 g of CuSO4?
Reaction: Na2S+ CuSO4 ⟶ Na2SO4 + CuS
A. 0.05
B. 9.58
C. 5.92
D. 15.45 - -B
Consider the following reaction: 2 Mg + O2 ⟶ 2 MgO Δ Hrxn = -1203 kJ. Calculate the
amount of heat (in kJ) associated with complete reaction of 4 moles of Mg.
A. -1203 kJ
, B. -601.5 kJ
C. -4812 kJ
D. None of the above
E. -2406 kJ - -E
Hydrochloric acid reacts with barium hydroxide according to the equation:
2 HCl (aq) + Ba(OH)2 (aq) ⟶ BaCl2 (aq) + 2 H2O ( l) Δ H= -118 kK
Calculate the heat (in kJ) associated with the complete reaction of 18.2 grams of HCl (aq).
A. -58.9
B. -29.5
C. None of above
D. -236
E. +58.9 - -B
How many grams of NO2 are theoretically produced if we start with 1.2 moles of S and 9.90
moles of HNO3?
