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Chapter 3: Problem 157

Which of the following statements about chemical equations is(are) true? a. When balancing a chemical equation, you can never change the coefficient in front of any chemical formula. b. The coefficients in a balanced chemical equation refer to the number of grams of reactants and products. c. In a chemical equation, the reactants are on the right and the products are on the left. d. When balancing a chemical equation, you can never change the subscripts of any chemical formula. e. In chemical reactions, matter is neither created nor destroyed so a chemical equation must have the same number of atoms on both sides of the equation.

Short Answer

Expert verified
Statements d and e are true. This is because when balancing a chemical equation, you should not change the subscripts of any chemical formula (Statement d), and in chemical reactions, the law of conservation of mass states that matter is neither created nor destroyed, requiring the same number of atoms for each element on both sides of the equation (Statement e).

Step by step solution

01

Statement a: Balancing a chemical equation by changing coefficients

Balancing a chemical equation involves adjusting the coefficients of the reactants and products to ensure that the number of atoms for each element is equal on both sides of the equation. Therefore, changing the coefficient in front of any chemical formula is acceptable when balancing a chemical equation. Statement a is false.
02

Statement b: Coefficients in a balanced chemical equation refer to grams

The coefficients in a balanced chemical equation represent the number of molecules or moles of reactants and products, not the number of grams. Statement b is false.
03

Statement c: Reactants on the right and products on the left

In a chemical equation, the reactants are typically written on the left side, while the products are written on the right side of the equation. The arrow separating them indicates the direction of the reaction. Statement c is false.
04

Statement d: Balancing a chemical equation by changing subscripts

When balancing a chemical equation, you should not change the subscripts of any chemical formula, as this would alter the identity of the compound. To balance the equation, you should only adjust the coefficients in front of the chemical formulas. Statement d is true.
05

Statement e: Matter conservation in chemical reactions

In chemical reactions, matter is conserved, meaning that the total number of atoms for each element must be the same on both sides of the equation. This principle is known as the law of conservation of mass. Statement e is true. In conclusion, statements d and e are true, while statements a, b, and c are false.

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Most popular questions from this chapter

Silicon is produced for the chemical and electronics industries by the following reactions. Give the balanced equation for each reaction. a. \(\mathrm{SiO}_{2}(s)+\mathrm{C}(s) \frac{\text { Electic }}{\text { arc furmae }} \mathrm{Si}(s)+\mathrm{CO}(g)\) b. Liquid silicon tetrachloride is reacted with very pure solid magnesium, producing solid silicon and solid magnesium chloride. c. \(\mathrm{Na}_{2} \mathrm{SiF}_{6}(s)+\mathrm{Na}(s) \rightarrow \operatorname{Si}(s)+\operatorname{NaF}(s)\)

Give the balanced equation for each of the following. a, The combustion of ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{OH}\right)\) forms carbon dioxide and water vapor. A combustion reaction refers to a reaction of a substance with oxygen gas. b. Aqueous solutions of lead(II) nitrate and sodium phosphate are mixed, resulting in the precipitate formation of lead(II) phosphate with aqueous sodium nitrate as the other product. c. Solid zinc reacts with aqueous \(\mathrm{HCl}\) to form aqueous zinc chloride and hydrogen gas. d. Aqueous strontium hydroxide reacts with aqueous hydrobromic acid to produce water and aqueous strontium bromide.

Bauxite, the principal ore used in the production of aluminum, has a molecular formula of \(\mathrm{Al}_{2} \mathrm{O}_{3} \cdot 2 \mathrm{H}_{2} \mathrm{O}\). The \(\cdot \mathrm{H}_{2} \mathrm{O}\) in the formula are called waters of hydration. Each formula unit of the compound contains two water molecules. a. What is the molar mass of bauxite? b. What is the mass of aluminum in \(0.58\) mole of bauxite? c. How many atoms of aluminum are in \(0.58\) mole of bauxite? d. What is the mass of \(2.1 \times 10^{24}\) formula units of bauxite?

A sample of a hydrocarbon (a compound consisting of only carbon and hydrogen) contains \(2.59 \times 10^{23}\) atoms of hydrogen and is \(17.3 \%\) hydrogen by mass. If the molar mass of the hydrocarbon is between 55 and \(65 \mathrm{~g} / \mathrm{mol}\), what amount (moles) of compound is present, and what is the mass of the sample?

Phosphorus can be prepared from calcium phosphate by the following reaction: \(2 \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s)+6 \mathrm{SiO}_{2}(s)+10 \mathrm{C}(s) \longrightarrow\) \(6 \mathrm{CaSiO}_{3}(s)+\mathrm{P}_{4}(s)+10 \mathrm{CO}(g)\) Phosphorite is a mineral that contains \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) plus other non-phosphorus- containing compounds. What is the maximum amount of \(\mathrm{P}_{4}\) that can be produced from \(1.0 \mathrm{~kg}\) of phosphorite if the phorphorite sample is \(75 \% \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) by mass? Assume an excess of the other reactants.
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