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CHEM111 Exam 2: Solutions and Reactions, Exams of Chemistry

Exam questions from a college-level chemistry course, focusing on topics such as calculating quantities of reactants and products, identifying reactants and oxidizing agents, and writing balanced net ionic equations. Questions include calculating the volume of a stock solution needed to prepare a given volume of a diluted solution, determining the mass of a product formed from given masses of reactants, identifying the species being oxidized and the oxidizing agent, calculating the enthalpy change for a reaction, and writing balanced net ionic equations for given reactions.

Typology: Exams

2010/2011

Uploaded on 10/17/2011

kelseybradley1
kelseybradley1 🇺🇸

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CHEM111, EXAM 2, S10 B Name_________________________________________
You must show all work for credit
1. (12 points) How many milliliters of a stock solution of 10.0 M HNO3 would you have to use to
prepare 0.350L of 0.400 M HNO3?
2. (12 points) Aluminum chloride is an inexpensive reagent used in many industrial processes. It is
made by treating scrap aluminum with chlorine according to the following reaction:
2 Al(s) + 3 Cl2(g) 2 AlCl3(s)
What mass of AlCl3 can be produced from 2.70 g of Al and 4.05 g of Cl2?
3. (6 points) In the following reaction:
Al(s) + 3 Ag+ Al3+ + Ag(s)
(a) identify the species being oxidized
(b) identify the oxidizing agent
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You must show all work for credit

  1. (12 points) How many milliliters of a stock solution of 10.0 M HNO 3 would you have to use to prepare 0.350L of 0.400 M HNO 3?
  2. (12 points) Aluminum chloride is an inexpensive reagent used in many industrial processes. It is made by treating scrap aluminum with chlorine according to the following reaction: 2 Al(s) + 3 Cl 2 (g) → 2 AlCl 3 (s)

What mass of AlCl 3 can be produced from 2.70 g of Al and 4.05 g of Cl 2?

  1. (6 points) In the following reaction: Al(s) + 3 Ag +^  Al 3+^ + Ag(s)

(a) identify the species being oxidized

(b) identify the oxidizing agent

You must show all work for credit

  1. (12 points) Calculate the Hrxn for the following reaction: Fe 2 O 3 (s) + 3 CO(g) → 2 Fe(s) + 3 CO 2 (g) Given the following: 2 Fe(s) + 3/2 O 2 (g) → Fe2O 3 (s) H = -824.2 kJ

CO(g) + ½ O 2 (g) → CO 2 (g) H = -282.7 kJ

  1. (16 points) Write balanced net ionic equations for the reactions that occur when each of the following solutions are mixed. If no reaction occurs write no reaction.

(a) sodium nitrate + magnesium bromide 

(b) sodium hydroxide + nickel(II) chloride 

(c) KOH + HCl 

(d) Na 2 CO 3 + MgCl (^2)

  1. (6 points) Write the chemical equation of the reaction for which the standard enthalpy change is equal to the standard enthalpy of formation for acetaminophen, C 8 H 9 O 2 N

You must show all work for credit

Potentially Helpful Information:

Substance Hf (kJ/mol)

H 2 S(g) -20. H 2 O(l) - H 2 O(g) - SO 2 (g) -296. SO 3 (g) -395.

Strong acids: HNO 3 , HCl, HBr, HI, H 2 SO 4 , HClO 4 and HClO 3

Solubility Rules :

  1. All lithium, sodium, potassium and ammonium salts are soluble.
  2. All salts containing nitrate and acetate are soluble.
  3. All salts containing chloride, bromide, and iodide are soluble except when also containing silver, lead(II) or mercury(I) ions.
  4. All salts containing sulfates are soluble except those which also contain lead(II), calcium, strontium, mercury(I) and barium.
  5. All hydroxides and metal oxides are insoluble except those of the group IA cations and those of calcium, strontium and barium.
  6. All phosphates, carbonates, sulfites and sulfides are insoluble except those of group IA cations or ammonium ion.