6. Chemical Quantities & Aqueous Reactions

Activity Series

6. Chemical Quantities & Aqueous Reactions

Activity Series

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Activity Series Example 1

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01:39

Metal Reactivity Series Menomics

Activity Series of Metals and Reaction Prediction

Lesson 29 - Activity Series, Part 1 (Chemistry Tutor)

8.3 Activity Series of the Elements

Reactivity Series of Metals | Environmental | Chemistry | FuseSchool

FuseSchool - Global Education

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Making Predictions Using Reactivity Series | Reactions | Chemistry | FuseSchool

04:08

Making Predictions Using Reactivity Series | Reactions | Chemistry | FuseSchool

FuseSchool - Global Education

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Predicting Products of Single Replacement Reactions

02:03

Predicting Products of Single Replacement Reactions

The Activity Series (Explanation & Examples)

Wayne Breslyn

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Open Question

Based on your understanding of activities determine if a reaction occurs and if so provide the products formed.

Ba (s) + H₂O (g) →

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Open Question

Based on your understanding of activities determine if a reaction occurs and if so provide the products formed.

Zn (s) + NiCl₂ (aq) →

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Open Question

If the activity of halogens is stated as:Fluorine > Chlorine > Bromine > Iodine, determine if a reaction occurs and if so provide the products formed.

Cl₂ (g) + AlBr₃ (aq) →

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Textbook Question

The most strongly reducing elements are listed at the top of the partial activity series table provided. Use the activity series to predict which reaction will occur. (LO 4.20) (a) (b) (c) (d)

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Textbook Question

Based on the positions in the periodic table, which of the following reactions would you expect to occur? (a) Red+ + Green ---> Red + Green+ (b) Blue + Green+ ---> Blue+ + Green (c) Red + Blue+ ---> Red+ + Blue

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Textbook Question

The following two redox reactions occur between aqueous cations and solid metals. Will a solution of green cations react with solid blue metal? Explain. (a)

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Textbook Question

Write balanced molecular and net ionic equations for the reactions of (d) aluminum with formic acid, HCOOH.

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Textbook Question

Write balanced molecular and net ionic equations for the reactions of (d) acetic acid, CH3COOH, with zinc.

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Textbook Question

Write balanced molecular and net ionic equations for the reactions of (b) dilute sulfuric acid with iron

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Textbook Question

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (b) zinc metal is added to a solution of magnesium sulfate

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Textbook Question

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (e) aluminum metal is added to a solution of cobalt(II) sulfate.

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Textbook Question

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (d) hydrogen gas is bubbled through an aqueous solution of nickel(II) chloride

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Textbook Question

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (c) hydrobromic acid is added to tin metal

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Textbook Question

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (e) hydrogen gas is bubbled through a solution of silver nitrate.

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Textbook Question

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (d) chromium metal is immersed in an aqueous solution of cobalt(II) chloride

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Textbook Question

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (b) a solution of zinc nitrate is added to a solution of magnesium sulfate

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Textbook Question

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (a) Nickel metal is added to a solution of copper(II) nitrate

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Textbook Question

The metal cadmium tends to form Cd2+ ions. The following observations are made: (i) When a strip of zinc metal is placed in CdCl21aq), cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in Ni1NO3221aq), nickel metal is deposited on the strip. (b) Which elements more closely define the position of cadmium in the activity series?

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Textbook Question

The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens: Br21aq2 + 2 NaI1aq2¡2 NaBr1aq2 + I21aq2 Cl21aq2 + 2 NaBr1aq2¡2 NaCl1aq2 + Br21aq2 (a) Which elemental halogen would you predict is the most stable, upon mixing with other halides?

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Textbook Question

Write the balanced chemical equation for the reaction of solid strontium with iodine gas.

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Textbook Question

Write the balanced chemical equation for the reaction of solid lithium with liquid water.

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Textbook Question

Write the balanced chemical equation for the reaction of solid potassium with liquid water.

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Textbook Question

Write the balanced equation for the reaction of hydrogen gas with bromine gas.

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Textbook Question

Assume that you are given a solution of an unknown acid or base. How can you tell whether the unknown substance is acidic or basic?

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Textbook Question

Consider the following reagents: zinc, copper, mercury (density 13.6 g/mL), silver nitrate solution, nitric acid solution. (a) Given a 500-mL Erlenmeyer flask and a balloon, can you combine two or more of the foregoing reagents to initiate a chemical reaction that will inflate the balloon? Write a balanced chemical equation to represent this process. What is the identity of the substance that inflates the balloon?

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Textbook Question

Bronze is a solid solution of Cu(s) and Sn(s); solutions of metals like this that are solids are called alloys. There is a range of compositions over which the solution is considered a bronze. Bronzes are stronger and harder than either copper or tin alone. (c) Suggest a reaction that you could do to remove all the tin from this bronze to leave a pure copper sample. Justify your reasoning.

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Textbook Question

Suppose you have 3.00 g of powdered zinc metal, 3.00g of powdered silver metal and 500.0 mL of a 0.2 M copper(II) nitrate solution. (d) What is the molarity of Cu2+ ions in the resulting solution?

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Textbook Question

Suppose you have 3.00 g of powdered zinc metal, 3.00g of powdered silver metal and 500.0 mL of a 0.2 M copper(II) nitrate solution. (a) Which metal will react with the copper(II) nitrate solution?

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Textbook Question

Determine whether HI can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HI and determine the minimum volume of 3.5 M HI required to completely dissolve the sample. c. 2.42gAg

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Textbook Question

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Textbook Question

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Textbook Question

Determine if HNO3 can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HNO3 and determine the minimum volume of 6.0 M HNO3 required to completely dissolve the sample. a. 5.90gAu

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Textbook Question

Use the activity series of metals (Table 4.5) to predict the outcome of each of the following reactions. If no reaction occurs, write NR. (d)

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Textbook Question

Use the activity series of metals (Table 4.5) to predict the outcome of each of the following reactions. If no reaction occurs, write NR. (c)

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Textbook Question

Use the activity series of metals (Table 4.5) to predict the outcome of each of the following reactions. If no reaction occurs, write NR. (b)

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Textbook Question

Use the activity series of metals (Table 4.5) to predict the outcome of each of the following reactions. If no reaction occurs, write NR. (a)

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Textbook Question

(b) Which of the following reactions would you expect to occur according to the activity series you established in part (a)?

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Textbook Question

(a) Use the following reactions to arrange the elements A, B, C, and D in order of their decreasing ability as reducing agents:

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Textbook Question

(a) Use the following reactions to arrange the elements A, B, C, and D in order of their decreasing ability as reducing agents:

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Textbook Question

(b) Which of the following reactions would you expect to occur according to the activity series you established in part (a)?

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Textbook Question

Chlorine dioxide gas 1ClO22 is used as a commercial bleaching agent. It bleaches materials by oxidizing them. In the course of these reactions, the ClO2 is itself reduced. (b) Why do you think that ClO2 is reduced so readily?

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Textbook Question

Some metals occur naturally in their elemental state while others occur as compounds in ores. Gold, for instance, is found as the free metal; mercury is obtained by heating mercury(II) sulfide ore in oxygen; and zinc is obtained by heating zinc(II) oxide ore with coke (carbon). Judging from their positions in the activity series, which of the metals sil-ver, platinum, and chromium would probably be obtained by (c) heating its oxide with coke?

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Textbook Question

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Textbook Question

A sample of metal (M) reacted with both steam and aqueous HCl to release H2 but did not react with water at room tem-perature. When 1.000 g of the metal was burned in oxygen, it formed 1.890 g of a metal oxide, M2O3. What is the iden-tity of the metal?

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Textbook Question

An unknown metal (M) was found not to react with either water or steam, but its reactivity with aqueous acid was not investigated. When a 1.000 g sample of the metal was burned in oxygen and the resulting metal oxide converted to a metal sulfide, 1.504 g of sulfide was obtained. What is the identity of the metal?

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Open Question

Nickel metal is added to a solution of copper(ii) nitrate.

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Open Question

Chromium metal is immersed in an aqueous solution of cobalt(ii) chloride.

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Open Question

What is produced during the replacement reaction of Cu(NO₃)₂ and Zn?

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Open Question

What will happen when a less reactive metal is added to a metal salt solution?

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6. Chemical Quantities & Aqueous Reactions

Activity Series

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