교과서 질문
Complete and balance the equation for each of the following reactions.
a. Fe(s) + H+(aq) →
c. Al(s)+ H+(aq) →
1
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Ch.22 - The Main Group Elements
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
22장, 문제 55
The hydrogen-filled dirigible Hindenburg had a volume of 1.99 * 108 L. If the hydrogen used was produced by the reaction of carbon with steam, how many kilograms of carbon would have been needed to produce enough hydrogen to fill the dirigible at 20 °C and 740 mm pressure?
검증된 단계별 안내1
Step 1: Write the balanced chemical equation for the reaction of carbon with steam to produce hydrogen gas. The reaction is typically represented as: \[ \text{C(s)} + \text{H}_2\text{O(g)} \rightarrow \text{CO(g)} + \text{H}_2(g) \].
Step 2: Use the ideal gas law to calculate the number of moles of hydrogen gas needed to fill the dirigible. The ideal gas law is given by \( PV = nRT \), where \( P \) is the pressure, \( V \) is the volume, \( n \) is the number of moles, \( R \) is the ideal gas constant, and \( T \) is the temperature in Kelvin.
Step 3: Convert the given temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature. Thus, \( T = 20 + 273.15 \).
Step 4: Convert the pressure from mmHg to atm, since the ideal gas constant \( R \) is typically given in terms of atm. Use the conversion factor: \( 1 \text{ atm} = 760 \text{ mmHg} \).
Step 5: Solve the ideal gas law equation for \( n \), the number of moles of hydrogen gas. Then, use stoichiometry from the balanced equation to determine the moles of carbon needed, and convert this to kilograms using the molar mass of carbon (12.01 g/mol).
주요 개념
질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.
Ideal Gas Law
The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is essential for calculating the amount of gas produced or required under specific conditions, such as the volume of hydrogen needed to fill the dirigible at given temperature and pressure.
추천 영상:
가이드 코스
01:15
Ideal Gas Law Formula
Stoichiometry
Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced equations. Understanding stoichiometry is crucial for determining how much carbon is needed to produce the required amount of hydrogen from the reaction of carbon with steam.
추천 영상:
가이드 코스
01:16Stoichiometry Concept
Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. It is important for converting between moles of a substance and its mass, allowing for the calculation of how many kilograms of carbon are necessary to produce the hydrogen needed for the dirigible.
추천 영상:
가이드 코스
02:11Molar Mass Concept