Stoichiometry Across the Courses

<-Homework Page Stoichiometry Problems Across the Courses: Practice Set by Ken Costello
The (x) are extra questions that I added to the textbook's question. Use other pages to show all work.

CHM130 textbook, Burns p331. prob.11.10	Lithium hydroxide can be used in closed environments such as the Space Shuttle and submarines to remove excess CO₂ gas. The unbalanced chemical equation is: LiOH(s) + CO₂(g) --> Li₂CO₃(s) + H₂O(g) If one CO₂ removal canister contains 250.g of LiOH(s), what mass of CO₂(g) will the canister be able to absorb? (x) Give the URL of a Web page that has an image of a carbon dioxide removal system.
CHM130 textbook, Burns p331. prob.11.11	Common antacids and dietary calcium supplements used to help prevent osteoporosis contain calcium carbonate. A CaCO₃ tablet dissolves in stomach acid, which contains hydrochloric acid. The unbalanced equation is: CaCO₃(s) + HCl(aq) --> CaCl₂(aq) + CO₂(g) + H₂O(l) What mass of HCl is required to react completely with the two tablets, each with 500.mg of CaCO₃?
CHM151 textbook, Silberberg, p128, prob.3.63	Potassium nitrate decomposes on heating, producing potassium oxide and gaseous nitrogen and oxygen. 4KNO₃(s) --> 2K₂O(s) + 2N₂(g) + 5O₂(g) To produce 88.6 kg of oxygen, how many (a) moles of KNO₃ must be heated? (b) Grams of KNO₃ must be heated? (x1) What does KNO₃ look like? (x2) KNO₃ is a component of gunpowder. What other two chemicals were present to make traditional gunpowder? (x3) What temperature does KNO₃ decompose?
CHM151 Silberberg, p128, prob. 3.67	Elemental phosphorus occurs as tetratomic molecules, P₄. (a) What mass of chlorine gas is needed to react completely with 355g of phosphorus to form phosphorus pentachloride? (x) What does elemental phosphorus look like?
CHM151 textbook, Silberberg, p128, prob. 3.70	Lead can be prepared from galena [Lead (II) sulfide] by first roasting the galena in oxygen gas to form lead (II) oxide and sulfur dioxide. In the second step, heating this lead (II) oxide with more galena forms molten lead and more sulfur dioxide. (a) Write a balanced equation for each step. (b) Write an overall balanced equation for the whole process (x1) If your car battery has 20 lbs of lead that came from galena, how many grams of sulfur dioxide was produced? (x2). What does galena look like?
CHM151LL lab Manual, p41, prob. 1, 2, 3, 4, 11, 14	Complete and balance each of the reactions. Declare them as acid/base neutralization, single replacement (redox), double replacement, combustion, decomposition, or combination (synthesis).
	P₂O₃ + H₂O --> H₃PO₄ C₄H₆ + O₂ --> H₂SO₄ + NH₄OH -->	FeCl₃ + AgNO₃ --> MgO + H₂O --> Mg(OH)₂ Zn + HCl -->
CHM151LL lab Manual, p153, prob. 2	Given a compound's molar mass (99 g/mol) and the element percent composition (by mass) is 48.5% C, 5.05%H, 14.1% N, and 32.3% O, determine the compound's molecular formula.
CHM152 textbook, p759 Silberberg,17.12	Balance each reaction and write its reaction quotient, Qc: (see page 727 for steps/p718 in 3rd edition) (a) NO(g) + O₂(g) <--> N₂O₃(g) (b) SF₆(g) + SO₃(g) <--> SO₂F₂(g)
CHM152 textbook, p952 Silberberg,21.13	Balance the following skeleton reaction & identify the oxidizing and reducing agents. (see pg 907/pg 897-3rd ed) O₂(g) + NO(g) --> NO₃^-(aq) (in an acidic solution)
CHM325 Analytical Chemistry textbook, 5-26.	A 0.1799g sample of an organic compound was burned in a stream of oxygen, and the CO₂ produced was collected in a solution of barium hydroxide. Calculate the moles of carbon in the sample if 0.5613g of BaCO₃ was formed. [FYI: Ba(OH)₂(aq) + CO₂(g)--> BaCO₃(s) + H₂O(l)]
CHM325, Analytical Chemistry textbook, 5-28.	The sulfur in an 8-tablet sample of the hypnotic drug captodiamine C₂₁H₂₉NS₂ (molar mass. 359.6 g/mol) was converted to sulfate and determined gravimetrically (the precipitate was weighed). Calculate the average mass of captodiamine per tablet if 0.3343 g of BaSO₄ was recovered.