When calcium comes in contact with water, calcium hydroxide and hydrogen gas is produced. 1. Justify why the above process is a chemical reaction. 2. Give the two pieces of evidence on the occurrence of the chemical reaction. 3. Write the word equation of the given reaction 4. Write the symbol equation

When calcium comes in contact with water, calcium hydroxide and hydrogen gas is produced. 1. Justify why the above process is a chemical reaction. 2. Give the two pieces of evidence on the occurrence of the chemical reaction. 3. Write the word equation of the given reaction 4. Write the symbol equation

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter13: Gases

Section13.10: Gas Stoichiometry

Problem 13.11SC: trong>Exercise 13.11 Calculate the volume of hydrogen produced at 1.50atmand 19Cby the reaction of...

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ercise 9.5 In Example 9.6 we answered one of the questions we posed in the introduction to this chapter. Now let’s see if you can answer the other question posed there. Determine what mass of carbon monoxide and what mass of hydrogen are required to form 6.0 kg of methanol by the reaction :math>CO(g)+2H2(g)CH3OH(l)
Exercise 6.3 Give the balanced equation for each of the following reactions.a. When solid ammonium nitrite is heated, it produces nitrogen gas and water vapor.b. Gaseous nitrogen monoxide (common name, nitric oxide) decomposes to produce dinitrogen monoxide gas (common name, nitrous oxide) and nitrogen dioxide gas.c. Liquid nitric acid decomposes to reddish-brown nitrogen dioxide gas. Liquid water, and oxygen gas. (This is why bottles of nitric acid become yellow upon standing.)
trong>Exercise 7.2 For each of the following reactions, write the molecular equation, the complete ionic equation, and the net ionic equation. ol type='a'> Aqueous sodium sulfide is mixed with aqueous copper(II) nitrate to produce solid copper(II) sulfide and aqueous sodium nitrate. i>Aqueous ammonium chloride and aqueous lead(ll) nitrate react to form solid lead(ll) chloride and aqueous ammonium nitrate.
ercise 9.1 Calculate the moles of CO2formed when 4.30 moles of C3H8reacts with the required 21.5 moles of O2. NT Use the moles of C3H8, and obtain the mole ratio between C3H8and CO2from the balanced equation.
You are given a sample of limestone, which is mostly CaCO3, to determine the mass percentage of Ca in the rock. You dissolve the limestone in hydrochloric acid, which gives a solution of calcium chloride. Then you precipitate the calcium ion in solution by adding sodium oxalate, Na2C2O4. The precipitate is calcium oxalate, CaC2O4. You find that a sample of limestone weighing 128.3 mg gives 140.2 mg of CaC2O4. What is the mass percentage of calcium in the limestone?
ercise 9.2 What mass of carbon dioxide is produced when 96.1 g of propane reacts with sufficient oxygen?
ercise 9.7 Titanium(IV) oxide is a white compound used as a coloring pigment. In fact, the pages in the hooks you read are white because of the presence of this compound in the paper. Solid titanium( IV) oxide can he prepared by reacting gaseous titanium( IV) chloride with oxygen gas. A second product of this reaction is chlorine gas. :math>TiCl4(g)+O2(g)TiO2(s)+Cl2(g) ppose 6.71103g of titanium(IV) chloride is reacted with 2.45103g of oxygen. Calculate the maximum mass of titanium(JV) oxide that can form.If the percent yield of TiO2 is 75%, what mass is actually formed?
ercise 9.4 Hydrofluoric acid, an aqueous solution containing dissolved hydrogen fluoride, is used to etch glass by reacting with the silica, SiO2, in the glass to produce gaseous silicon tetra fluoride and liquid water. The unbalanced equation is :math>HF(aq)+SiO2(s)SiF4(g)+H2O(l) l type='a'> Calculate the mass of hydrogen fluoride needed to react with 5.68 g of silica. Hint: Think carefully about this problem. What is the balanced equation for the reaction? What is given? What do you need to calculate? Sketch a map of the problem before you do the calculations. Calculate the mass of water produced in the reaction described in part a.
Sodium is a soft, reactive metal that instantly reacts with water to give hydrogen gas and a solution of sodium hydroxide, NaOH. How many grams of sodium metal are needed to give 7.81 g of hydrogen by this reaction? (Remember to write the balanced equation first.)
trong>Exercise 13.11 Calculate the volume of hydrogen produced at 1.50atmand 19Cby the reaction of 26.5gof zinc with excess hydrochloric acid according to the balanced equation msp;Zn(s)+2HCl(aq)ZnCl2(aq)+H2(g)
Aluminum chloride, AlCl3, is used as a catalyst in various industrial reactions. It is prepared from hydrogen chloride gas and aluminum metal shavings. 2Al(s)+6HCl(g)2AlCl3(s)+3H2(g) Suppose a reaction vessel contains 0.15 mol Al and 0.35 mol HCl. How many moles of AlCl3 can be prepared from this mixture?
Exercise19.3Watches with numerals that glow in the dark” formerly were made by including radioactive radium in the paint used to letter the watch faces. Assume that to make the numeral 3 on a given watch, a sample of paint containing8.0107 mole ofR88228a was used. This watch was then put in a drawer and forgotten. Many years later someone finds the watch and wishes to know when it was made. Analyzing the paint, this person finds1.0107 moles ofR88228a in the numeral 3. Flow much time elapsed between the making of the watch and the finding of the watch? Watches and clocks with radium dials.

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