/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 167 Which of the following statement... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 3: Problem 167

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
The true statements about chemical equations are: - Statement d: When balancing a chemical equation, you can never change the subscripts of any chemical formula. - Statement 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.

Step by step solution

01

Statement a: Balancing chemical equations and coefficients.

Statement a states that when balancing a chemical equation, we can never change the coefficient in front of any chemical formula. This statement is actually false. When balancing a chemical equation, we need to adjust the coefficients in front of the chemical formulas to ensure that the number of atoms of each element is the same on both sides of the equation. So, changing coefficients is crucial for balancing chemical equations.
02

Statement b: Coefficients and grams of reactants and products

Statement b says that the coefficients in a balanced chemical equation refer to the number of grams of reactants and products. This statement is incorrect. Coefficients in a balanced chemical equation refer to the number of molecules or moles (not grams) of the reactants and products involved in the chemical reaction.
03

Statement c: Reactants and products in a chemical equation

Statement c proposes that in a chemical equation, the reactants are on the right and the products are on the left. This statement is false. In a chemical equation, the reactants are typically written on the left side and the products are written on the right side of the equation. The reactants and products are separated by an arrow pointing towards the products.
04

Statement d: Balancing chemical equations and subscripts

Statement d claims that when balancing a chemical equation, we can never change the subscripts of any chemical formula. This statement is true. We should not change the subscripts while balancing a chemical equation, as altering the subscripts would change the identity of the compounds involved in the reaction. Instead, we should adjust the coefficients to balance the equation.
05

Statement e: Matter conservation in chemical reactions

Statement e mentions that 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. This statement is true. This is based on the law of conservation of mass, which states that the total mass of the reactants must be equal to the total mass of the products in a chemical reaction. Balancing the chemical equation ensures that the same number of atoms is present on both sides of the equation, thus conserving the mass. In conclusion, the true statements about chemical equations are: - Statement d: When balancing a chemical equation, you can never change the subscripts of any chemical formula. - Statement 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.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

An element consists of 1.40\(\%\) of an isotope with mass 203.973 u, 24.10\(\%\) of an isotope with mass 205.9745 u, 22.10\(\%\) of an isotope with mass 206.9759 u, and 52.40\(\%\) of an isotope with mass 207.9766 u. Calculate the average atomic mass, and identify the element.

An ionic compound \(\mathrm{MX}_{3}\) is prepared according to the following unbalanced chemical equation. $$ \mathrm{M}+\mathrm{X}_{2} \longrightarrow \mathrm{MX}_{3} $$ A 0.105 -g sample of \(\mathrm{X}_{2}\) contains \(8.92 \times 10^{20}\) molecules. The compound \(\mathrm{MX}_{3}\) consists of 54.47\(\% \mathrm{X} \mathrm{by}\) mass. What are the identities of \(\mathrm{M}\) and \(\mathrm{X}\) , and what is the correct name for \(\mathrm{MX}_{3} ?\) Starting with 1.00 \(\mathrm{g}\) each of \(\mathrm{M}\) and \(\mathrm{X}_{2},\) what mass of \(\mathrm{MX}_{3} \mathrm{can}\) be prepared?

A 0.755 -g sample of hydrated copper(II) sulfate $$ \mathrm{CuSO}_{4} \cdot x \mathrm{H}_{2} \mathrm{O} $$ was heated carefully until it had changed completely to anhydrous copper(II) sulfate \(\left(\mathrm{CuSO}_{4}\right)\) with a mass of 0.483 g. Determine the value of \(x .[\text { This number is called the number of waters }\) of hydration of copper(Il) sulfate. It specifies the number of water molecules per formula unit of \(\mathrm{CuSO}_{4}\) in the hydrated crystal. \(]\)

Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid-fuel rocket motors. The reaction is $$ \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+2 \mathrm{Al}(s) \longrightarrow 2 \mathrm{Fe}(l)+\mathrm{Al}_{2} \mathrm{O}_{3}(s) $$ What masses of iron(III) oxide and aluminum must be used to produce 15.0 \(\mathrm{g}\) iron? What is the maximum mass of aluminum oxide that could be produced?

The reaction between potassium chlorate and red phosphorus takes place when you strike a match on a matchbox. If you were to react 52.9 g of potassium chlorate \(\left(\mathrm{KClO}_{3}\right)\) with excess red phosphorus, what mass of tetraphosphorus decaoxide \(\left(\mathrm{P}_{4} \mathrm{O}_{10}\right)\) could be produced? \(\mathrm{KClO}_{3}(s)+\mathrm{P}_{4}(s) \longrightarrow \mathrm{P}_{4} \mathrm{O}_{10}(s)+\mathrm{KCl}(s) \quad\) (unbalanced)
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Kinetics

Read Explanation

Chemical Reactions

Read Explanation

Nuclear Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Making Measurements

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.