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Chapter 14: Problem 78

Complete and balance the following: (a) \(\mathrm{H}_{2} \mathrm{~S}(g)+\mathrm{O}_{2}(g) \longrightarrow\) (b) \(\mathrm{SO}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (c) \(\mathrm{SF}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(I) \longrightarrow\) (d) \(\mathrm{Al}_{2} \mathrm{Se}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\)

Short Answer

Expert verified
(a) \text{2}\text{H}_{2}\text{S}(g) + \text{3}\text{O}_{2}(g) \rightarrow 2\text{H}_{2}\text{O}(g) + 2\text{SO}_{2}(g)(b) \text{SO}_{3}(g) + \text{H}_{2}\text{O}(l) \rightarrow \text{H}_{2}\text{SO}_{4}(aq)(c) \text{SF}_{4}(g) + 3\text{H}_{2}\text{O}(l) \rightarrow \text{H}_{2}\text{SO}_{3}(aq) + \text{4HF}(aq)(d) \text{Al}_{2}\text{Se}_{3} (s) + 6\text{H}_{2}\text{O}(l) \rightarrow 2\text{Al}\text{(OH)}_{3}(s) + 3\text{H}_{2}\text{Se}(g)

Step by step solution

01

Identify reactants and predicted products for each reaction

For each equation, identify the reactants and predict the products based on chemical reactivity and typical synthesis or decomposition reactions.
02

Complete the reactions

Predict the products for each reaction based on commonly known chemical reactions and write down the unbalanced equations.
03

Balance the equations

Adjust the coefficients of each reactant and product to ensure that the number of atoms for each element is equal on both sides of the equation.
04

Write the balanced equations

Rewrite each equation ensuring that the coefficients balance the number of atoms of each element on both sides of the equations.

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Key Concepts

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

chemical reactions
Chemical reactions are processes where reactants transform into products. Think of it as rearranging Lego bricks to create something new. Reactants are the starting materials and products are what you end up with after the transformation. Reactions can be classified into several types such as synthesis, decomposition, single displacement, and double displacement. Understanding these types helps in predicting the products.
reaction balancing
Balancing chemical equations is crucial because it ensures the law of conservation of mass is followed. This law states that matter cannot be created or destroyed in a chemical reaction. To balance an equation, you adjust the coefficients (numbers in front of molecules) to make sure the number of each type of atom is the same on both the reactant and product sides. Start by balancing elements that appear only once on each side, then move to more complex ones.
stoichiometry
Stoichiometry is about the quantitative relationships in chemical reactions, allowing us to predict how much of each substance is needed or formed. Using balanced equations, you can calculate the moles, mass, and volumes of reactants and products. The key is to use the coefficients from the balanced equation to set up mole ratios. This helps in scaling reactions up or down and ensures the correct amounts for practical applications.
predicting products
Predicting the products of a chemical reaction involves knowing the types of reactions and the reactivity of different substances. For instance, combining an acid with a base typically produces water and a salt. Recognizing patterns in reaction types, such as synthesis or decomposition, helps predict the outcomes. Familiarity with ions and compounds' properties also aids in accurately guessing the products of new reactions.

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Most popular questions from this chapter

Two substances with the empirical formula HNO are hyponitrous acid \((\mathscr{A}=62.04 \mathrm{~g} / \mathrm{mol})\) and nitroxyl \((\mathscr{A}=31.02 \mathrm{~g} / \mathrm{mol}) .\) (a) What is the molecular formula of each species? (b) For each species, draw the Lewis structure having the lowest formal charges. (Hint: Hyponitrous acid has an \(\mathrm{N}=\mathrm{N}\) bond. \()\) (c) Predict the shape around the \(\mathrm{N}\) atoms of each species. (d) When hyponitrous acid loses two protons, it forms the hyponitrite ion. Draw cis and trans forms of this ion.

Compounds such as \(\mathrm{NaBH}_{4}, \mathrm{Al}\left(\mathrm{BH}_{4}\right)_{3},\) and \(\mathrm{LiAlH}_{4}\) are com- plex hydrides used as reducing agents in many syntheses. (a) Give the oxidation state of each element in these compounds. (b) Write a Lewis structure for the polyatomic anion in \(\mathrm{NaBH}_{4}\), and predict its shape.

Indium (In) reacts with \(\mathrm{HCl}\) to form a diamagnetic solid with the formula \(\ln \mathrm{Cl}_{2}\). (a) Write condensed electron configurations for \(\mathrm{In}, \mathrm{In}^{+}, \mathrm{In}^{2+}\) and \(\mathrm{In}^{3+}\) (b) Which of these species is (are) diamagnetic and which paramagnetic? (c) What is the apparent oxidation state of In in \(\mathrm{InCl}_{2}\) ? (d) Given your answers to parts (b) and (c), explain how \(\mathrm{InCl}_{2}\) can be diamagnetic.

Even though EN values vary relatively little down Group \(4 \mathrm{~A}(14),\) the elements change from nonmetal to metal. Explain.

Assuming acid strength relates directly to number of \(\mathrm{O}\) atoms bonded to the central atom, rank \(\mathrm{H}_{2} \mathrm{~N}_{2} \mathrm{O}_{2}\left[\mathrm{or}(\mathrm{HON})_{2}\right], \mathrm{HNO}_{3}\) (or HONO \(_{2}\) ), and \(\mathrm{HNO}_{2}\) (or HONO) in order of decreasing acid strength.
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