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Chapter 7: Problem 37

Balance each of the following chemical equations: a. \(\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{NO}(g)\) b. \(\mathrm{HgO}(s) \stackrel{\Delta}{\longrightarrow} \mathrm{Hg}(l)+\mathrm{O}_{2}(g)\) c. \(\mathrm{Fe}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{Fe}_{2} \mathrm{O}_{3}(s)\) d. \(\mathrm{Na}(s)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{NaCl}(s)\)

Short Answer

Expert verified
a) \(\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2\mathrm{NO}(g)\), b) 2\mathrm{HgO}(s) \stackrel{\Delta}{\longrightarrow} 2\mathrm{Hg}(l)+\mathrm{O}_{2}(g)\), c) \(4\mathrm{Fe}(s)+3\mathrm{O}_{2}(g) \longrightarrow 2\mathrm{Fe}_{2}\mathrm{O}_{3}(s)\), d) 2\mathrm{Na}(s)+\mathrm{Cl}_{2}(g) \longrightarrow 2\mathrm{NaCl}(s)\)

Step by step solution

01

Write the Skeleton Equations

Write down the unbalanced chemical equations for each problem:a. \(\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{NO}(g)\) b. \(\mathrm{HgO}(s) \stackrel{\Delta}{\longrightarrow} \mathrm{Hg}(l)+\mathrm{O}_{2}(g)\) c. \(\mathrm{Fe}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{Fe}_{2}\mathrm{O}_{3}(s)\) d. \(\mathrm{Na}(s)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{NaCl}(s)\)
02

Balance the Elements Already Combined in Compounds First (a)

For \(\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{NO}(g)\), we start with nitrogen. There are 2 nitrogen atoms on the left side and 1 on the right. Multiply \(\mathrm{NO}\) by 2 to balance nitrogen: \(\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2\mathrm{NO}(g)\).Then, count the oxygen atoms: there are now 2 oxygen atoms on both sides.
03

Balance the Elements Already Combined in Compounds First (b)

For \(\mathrm{HgO}(s) \stackrel{\Delta}{\longrightarrow} \mathrm{Hg}(l)+ \mathrm{O}_{2}(g)\), start with mercury. There is 1 mercury atom on each side, so it is balanced. Next, balance oxygen by multiplying \(\mathrm{HgO}\) by 2: \(2\mathrm{HgO}(s) \stackrel{\Delta}{\longrightarrow} 2\mathrm{Hg}(l) + \mathrm{O}_{2}(g)\).Now, there are 2 oxygen atoms on each side.
04

Balance the Elements Already Combined in Compounds First (c)

For \(\mathrm{Fe}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{Fe}_{2}\mathrm{O}_{3}(s)\), balance iron by multiplying \(\mathrm{Fe}\) by 2: \(2\mathrm{Fe}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{Fe}_{2}\mathrm{O}_{3}(s)\).Next, balance oxygen. There are 3 oxygens on the right, so multiply \(\mathrm{O}_{2}\) by 3/2. Since we should use whole numbers, multiply all coefficients by 2 to get the final balanced equation: \(4\mathrm{Fe}(s)+3\mathrm{O}_{2}(g) \longrightarrow 2\mathrm{Fe}_{2}\mathrm{O}_{3}(s)\).
05

Balance the Elements Already Combined in Compounds First (d)

For \(\mathrm{Na}(s)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{NaCl}(s)\), balance sodium by putting a coefficient of 2 before \(\mathrm{NaCl}\): \(\mathrm{Na}(s)+\mathrm{Cl}_{2}(g) \longrightarrow 2\mathrm{NaCl}(s)\).Next, balance chlorine by putting a coefficient of 2 before \(\mathrm{Na}\): \(2\mathrm{Na}(s)+\mathrm{Cl}_{2}(g) \longrightarrow 2\mathrm{NaCl}(s)\).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Stoichiometry
Stoichiometry is a key concept for understanding how reactants and products relate in a chemical reaction. It involves using balanced chemical equations to calculate the amounts of reactants and products.

For example, in the balanced equation for the reaction between nitrogen and oxygen to form nitric oxide: \(\text{N}_{2}(g)+\text{O}_{2}(g) \rightarrow 2\text{NO}(g)\), \we can see that one molecule of nitrogen reacts with one molecule of oxygen to produce two molecules of nitric oxide.

This tells us the exact ratio in which substances react, which is crucial for determining how much of each substance is needed or produced.
  • To balance a chemical equation, first write the unbalanced equation.
  • Balance the atoms that appear in only one reactant and one product first.
  • Adjust coefficients to get the same number of each type of atom on both sides.
  • Always use the smallest whole numbers as coefficients.
Law of Conservation of Mass
The law of conservation of mass states that mass is neither created nor destroyed in a chemical reaction. This means the total mass of reactants must equal the total mass of products.

In the exercise, when balancing the equation \(2\text{HgO}(s) \rightarrow 2\text{Hg}(l) + \text{O}_{2}(g)\), \you ensure that the number of Hg and O atoms are the same on both sides.

This law is why balancing chemical equations is so important. If atoms are not balanced:
  • The equation doesn't accurately represent the reaction.
  • It would violate the conservation of mass.


So, always count each type of atom on both sides of the equation and adjust the coefficients to balance them.
Chemical Reactions
Chemical reactions involve the rearrangement of atoms to form new substances. The substances reacting are called reactants, and the new substances formed are products.

There are several types of chemical reactions, including:
  • Synthesis reactions: Two or more simple substances combine to form a more complex substance. Example: \(2\text{Na}(s) + \text{Cl}_{2}(g) \rightarrow 2\text{NaCl}(s) \)
  • Decomposition reactions: A complex substance breaks into two or more simpler substances. Example: \(2\text{HgO}(s) \rightarrow 2\text{Hg}(l) + \text{O}_{2}(g) \)
  • Single replacement reactions: One element replaces another in a compound.
  • Double replacement reactions: Two compounds exchange elements.


Understanding these types can help predict what products will form in a reaction and how to balance the equations.

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Most popular questions from this chapter

During heavy exercise and workouts, lactic acid, \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}_{3}\), accumulates in the muscles where it can cause pain and soreness. (7.1,7.2) a. How many molecules are in 0.500 mole of lactic acid? b. How many atoms of \(\mathrm{C}\) are in 1.50 moles of lactic acid? c. How many moles of lactic acid contain \(4.5 \times 10^{24}\) atoms of \(\mathrm{O} ?\) d. What is the molar mass of lactic acid?

Sodium reacts with oxygen to produce sodium oxide. $$ 4 \mathrm{Na}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Na}_{2} \mathrm{O}(s) $$ a. How many grams of \(\mathrm{Na}_{2} \mathrm{O}\) are produced when \(57.5 \mathrm{~g}\) of Na reacts? b. If you have \(18.0 \mathrm{~g}\) of \(\mathrm{Na}\), how many grams of \(\mathrm{O}_{2}\) are needed for the reaction? c. How many grams of \(\mathrm{O}_{2}\) are needed in a reaction that produces \(75.0 \mathrm{~g}\) of \(\mathrm{Na}_{2} \mathrm{O} ?\)

a. How does a catalyst affect the activation energy? b. Why is pure oxygen used in respiratory distress?

Calculate the molar mass for each of the following: a. \(\mathrm{O}_{2}\) b. \(\mathrm{KH}_{2} \mathrm{PO}_{4}\) c. \(\mathrm{Fe}\left(\mathrm{ClO}_{4}\right)_{3}\)

Aluminum sulfate, \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3},\) is used in some antiperspirants. a. How many moles of \(\mathrm{O}\) are present in \(3.0 \mathrm{moles}\) of \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} ?\) b. How many moles of aluminum ions \(\left(\mathrm{Al}^{3+}\right)\) are present in 0.40 mole of \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} ?\) c. How many moles of sulfate ions \(\left(\mathrm{SO}_{4}^{2-}\right)\) are present in 1.5 moles of \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} ?\)
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