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Chapter 3: Problem 40

Balance the following equations: (a) \(\mathrm{SiCl}_{4}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{SiO}_{2}+\mathrm{HCl}\) (b) \(\mathrm{P}_{4} \mathrm{O}_{10}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{H}_{3} \mathrm{PO}_{4}\) (c) \(\mathrm{CaCN}_{2}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{CaCO}_{3}+\mathrm{NH}_{3}\) (d) \(\mathrm{NO}_{2}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{HNO}_{3}+\mathrm{NO}\)

Short Answer

Expert verified
(a) SiCl4 + 2 H2O -> SiO2 + 4 HCl, (b) P4O10 + 6 H2O -> 4 H3PO4, (c) CaCN2 + 3 H2O -> CaCO3 + 2 NH3, (d) 3 NO2 + H2O -> 2 HNO3 + NO.

Step by step solution

01

Balance SiCl4 + H2O -> SiO2 + HCl

Identify the number of each type of atom on both sides of the equation. Start with silicon: there's 1 Si on each side, so they're balanced. For chlorine (Cl), there are 4 Cl in SiCl4 and on the product side, as each HCl contains 1 Cl, we need 4 HCl. To balance hydrogen, now with 4 H in HCl, we need 2 H2O to provide 4 H. Oxygen is balanced since each side has 2 O atoms: \( \text{SiCl}_4 + 2 \text{H}_2\text{O} \rightarrow \text{SiO}_2 + 4 \text{HCl} \).
02

Balance P4O10 + H2O -> H3PO4

For phosphorus, on the reactant side, we start with 4 P, so we need 4 H3PO4 molecules to balance phosphorus. Oxygen in P4O10 contributes 10, and 4 H3PO4 contains 16 oxygens; thus, 6 oxygens must come from water, indicating we need 6 H2O. This adjustment balances the hydrogen as well, with a total of 12 H from 6 H2O:\( \text{P}_4\text{O}_{10} + 6 \text{H}_2\text{O} \rightarrow 4 \text{H}_3\text{PO}_4 \).
03

Balance CaCN2 + H2O -> CaCO3 + NH3

Calcium is already balanced since there's 1 Ca on each side. Carbon is initially unbalanced, with 2 C on the left and only 1 in CaCO3 on the right. Since NH3 contains nitrogen, and there's 2 N in CaCN2, we need two NH3 molecules, which provides 2 H from water. Using 2 H2O yields the 2 O atoms needed for CaCO3:\( \text{CaCN}_2 + 3 \text{H}_2\text{O} \rightarrow \text{CaCO}_3 + 2 \text{NH}_3 \).
04

Balance NO2 + H2O -> HNO3 + NO

Start with nitrogen, which is balanced since each side has 1 N per NO2, HNO3, and NO. For oxygen, we note each NO2 has 2 O, requiring additional O from water to produce both HNO3 and NO, which results in 3 O from products: 1 from NO and 2 from HNO3 each. Using 1 H2O balances oxygen and hydrogen:\( 3 \text{NO}_2 + \text{H}_2\text{O} \rightarrow 2 \text{HNO}_3 + \text{NO} \).

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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 in chemistry that involves using relationships between reactants and products in a chemical reaction to find the exact amount of substances involved. It serves as a bridge to help us convert moles of one substance to moles of another through the balanced chemical equation.
For example, if we look at the chemical reaction of combusting methane - CH extsubscript{4} + 2O extsubscript{2} -> CO extsubscript{2} + 2H extsubscript{2}O, stoichiometry allows us to predict that 2 moles of water will be produced for every mole of methane burned.
  • **Mole Ratios:** The coefficients in a balanced equation reflect the proportions (mole ratios) required for the reactants and products. This relationship is central to calculating various quantities.
  • **Mass and Mole Conversions:** Knowing the molar mass of compounds allows for the conversion between grams of a substance and moles, making stoichiometry calculations possible.
  • **Limiting Reactants:** Stoichiometry helps identify which reactant will run out first, thus limiting the amount of product formed in reactions.
By carefully tracking moles and masses, stoichiometry ensures that chemical instructions are followed precisely.
Chemical Reactions
Chemical reactions are processes where substances, known as reactants, are transformed into different substances termed as products. This occurs via breaking and forming of bonds which leads to new compound structures.
  • **Types of Reactions:** There are several types of chemical reactions including synthesis, decomposition, single-replacement, double-replacement, and combustion. Each type has a unique pattern of reactant and product formation.
  • **Reaction Conditions:** Various factors such as temperature, pressure, and the presence of catalysts can affect the rate and outcome of chemical reactions.
  • **Conservation of Mass:** In a chemical reaction, the mass of the reactants equals the mass of the products. This is due to the law of conservation of mass which states matter is neither created nor destroyed.
Grasping the nature of these reactions helps in not just predicting the products, but also understanding natural and industrial processes.
Balancing Chemical Equations
Balancing chemical equations ensures that the same number of each type of atom appears on both sides of the equation, reflecting the conservation of matter. Each chemical equation must obey this principle to be physically meaningful.
Balancing involves:
  • **Identifying Elements:** First, determine each element present in the equation and count how many atoms they currently have on each side.
  • **Adjusting Coefficients:** You adjust the coefficients (the numbers in front of molecules) to ensure every element matches on both sides of the arrow. Often, starting with the most complex molecule makes it easier.
  • **Iterative Process:** It's a bit of trial and error. Sometimes you'll need to readjust as adding coefficients to one compound might throw off the balance elsewhere in the equation.
The result is that the balanced equation provides accurate stoichiometric ratios, enabling precise predictions and calculations in chemical reactions.

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Most popular questions from this chapter

Coniine, a toxic substance isolated from poison hemlock, contains only carbon, hydrogen, and nitrogen. Combustion analysis of a \(5.024 \mathrm{mg}\) sample yields \(13.90 \mathrm{mg}\) of \(\mathrm{CO}_{2}\) and \(6.048 \mathrm{mg}\) of \(\mathrm{H}_{2} \mathrm{O}\). What is the empirical formula of coniine?

What is the molecular weight of chloroform if \(0.0275 \mathrm{~mol}\) weighs \(3.28 \mathrm{~g}\) ?

Cytochrome \(c\) is an iron-containing enzyme found in the cells of all aerobic organisms. If cytochrome \(c\) is \(0.43 \%\) Fe by mass, what is its minimum molecular weight?

Cisplatin \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\right]\), a compound used in cancer treatment, is prepared by reaction of ammonia with potassium tetrachloroplatinate: $$ \mathrm{K}_{2} \mathrm{PtCl}_{4}+2 \mathrm{NH}_{3} \longrightarrow 2 \mathrm{KCl}+\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2} $$ How many grams of cisplatin are formed from \(55.8 \mathrm{~g}\) of \(\mathrm{K}_{2} \mathrm{PtCl}_{4}\) and \(35.6 \mathrm{~g}\) of \(\mathrm{NH}_{3}\) if the reaction takes place in \(95 \%\) yield based on the limiting reactant?

When a diabetic experiences low blood glucose, possibly due to an excess of insulin or increased levels of exercise, the treatment is consumption of glucose tablets. (a) How many grams of glucose are in the recommended amount for treatment of an adult, \(0.0833\) mol glucose? (b) A typical tablet contains \(3.75 \mathrm{~g}\) of glucose. How many tablets should be eaten? (c) How many molecules of glucose are in \(0.0833\) mol?
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