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Get Full Access to Chemistry: The Central Science - 14 Edition - Chapter 3 - Problem 3.11
Get Full Access to Chemistry: The Central Science - 14 Edition - Chapter 3 - Problem 3.11

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# ?Balance the following equations: (a) $$\mathrm{CO}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)$$ (b) $$\mathrm{N}_{2} \ ISBN: 9780134414232 1274 ## Solution for problem 3.11 Chapter 3 Chemistry: The Central Science | 14th Edition • Textbook Solutions • 2901 Step-by-step solutions solved by professors and subject experts • Get 24/7 help from StudySoup virtual teaching assistants Chemistry: The Central Science | 14th Edition 4 5 1 325 Reviews 14 1 Problem 3.11 Balance the following equations: (a) \(\mathrm{CO}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)$$

(b) $$\mathrm{N}_{2} \mathrm{O}_{5}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{HNO}_{3}(a q)$$

(c) $$\mathrm{CH}_{4}(g)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{CCl}_{4}(l)+\mathrm{HCl}(g)$$

(d) $$\mathrm{Zn}(\mathrm{OH})_{2}(s)+\mathrm{HNO}_{3}(a q) \longrightarrow \mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$$

Text Transcription:

CO(g)+ O_2(g) \longrightarrow CO_2(g)

N_2 O_5(g)+H_2O(l) \longrightarrow HNO_3(a q)

CH_4(g)+Cl_2(g) \longrightarrow CCl_{4}(l)+HCl(g)

Zn(OH)_2(s)+HNO_{(a q) \longrightarrow Zn(NO_3)_2(a q)+H_2 O(l)

Step-by-Step Solution:

Step 1 of 5) The second line in the table (Change) summarizes the amounts of reactants consumed (where this consumption is indicated by the minus signs) and the amount of the product formed (indicated by the plus sign). These quantities are restricted by the quantity of the limiting reactant and depend on the coefficients in the balanced equation. The mole ratio H2:O2:H2O = 10:5:10 is a multiple of the ratio of the coefficients in the balanced equation, 2:1:2. The after quantities, which depend on the before quantities and their changes, are found by adding the before quantity and change quantity for each column. The amount of the limiting reactant 1H22 must be zero at the end of the reaction. What remains is 2 mol O2 (excess reactant) and 10 mol H2O (product).Analyze We are asked to calculate the number of moles of product, NH3, given the quantities of each reactant, N2 and H2, available in a reaction. This is a limiting reactant problem. Plan If we assume one reactant is completely consumed, we can calculate how much of the second reactant is needed. By comparing the calculated quantity of the second reactant with the amount available, we can determine which reactant is limiting. We then proceed with the calculation, using the quantity of the limiting reactant.

Step 2 of 2

##### ISBN: 9780134414232

This textbook survival guide was created for the textbook: Chemistry: The Central Science, edition: 14. This full solution covers the following key subjects: . This expansive textbook survival guide covers 29 chapters, and 2820 solutions. Chemistry: The Central Science was written by and is associated to the ISBN: 9780134414232. The answer to “?Balance the following equations: (a) $$\mathrm{CO}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)$$(b) $$\mathrm{N}_{2} \mathrm{O}_{5}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{HNO}_{3}(a q)$$(c) $$\mathrm{CH}_{4}(g)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{CCl}_{4}(l)+\mathrm{HCl}(g)$$(d) $$\mathrm{Zn}(\mathrm{OH})_{2}(s)+\mathrm{HNO}_{3}(a q) \longrightarrow \mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$$Text Transcription:CO(g)+ O_2(g) \longrightarrow CO_2(g)N_2 O_5(g)+H_2O(l) \longrightarrow HNO_3(a q)CH_4(g)+Cl_2(g) \longrightarrow CCl_{4}(l)+HCl(g)Zn(OH)_2(s)+HNO_{(a q) \longrightarrow Zn(NO_3)_2(a q)+H_2 O(l)” is broken down into a number of easy to follow steps, and 38 words. Since the solution to 3.11 from 3 chapter was answered, more than 219 students have viewed the full step-by-step answer. The full step-by-step solution to problem: 3.11 from chapter: 3 was answered by , our top Chemistry solution expert on 10/03/18, 06:29PM.

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?Balance the following equations: (a) $$\mathrm{CO}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)$$ (b) \(\mathrm{N}_{2} \