Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
"Heater meals" are precooked meals that come with a water-activated heating mechanism. One way to heat a meal is to pour water on magnesium:
Mg(s) + 2 H2O(l) → Mg(OH)2(s) + H2(g)
This reaction releases 352.88 kJ as written above.
Assuming magnesium is the limiting reactant, how many kilojoules of energy will be released if one starts with 2.50 g Mg? Don't include units in the box with your answer.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 2 steps with 1 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- MISSED THIS? Watch KCV 9.6, IWE 9.7; Read Section 9.6. You can click on the Review link to access the section in your eText. Titanium reacts with iodine to form titanium(III) iodide, emitting heat, via the following reaction: 2Ti(s) +31₂(g)→2Til3 (s), AHxn = -839 kJ Part A Determine the mass of titanium that reacts if 1.60×10³ kJ of heat is emitted by the reaction. Express your answer to three significant figures and include the appropriate units. µÅ m(Ti) = Submit Part B Value X Incorrect; Try Again; 2 attempts remaining m(l₂)= Submit Previous Answers Request Answer Determine the mass of iodine that reacts if 1.60×10³ kJ of heat is emitted by the reaction. Express your answer to three significant figures and include the appropriate units. Units 0 O µÂ Value Units Previous Answers Request Answer ? X Incorrect; Try Again; 2 attempts remaining ?arrow_forwardWhen 40 mL of 1.0 M HCl was mixed with 50 mL of 1.5 M NaOH in a coffee cup calorimeter, the temperature of the solution rose from 24.8 C to 41.5 C. Determine the heat of the reaction. Is the reaction endothermic or exothermic? Explain.arrow_forwardHow much energy is required to decompose 1970 g of PCl3, according to the reaction below? 4 PCl3(g) → P4(s) + 6 Cl2(g) ΔH°RXN = +1207 kJarrow_forward
- In a constant-pressure calorimeter, 55.0 mL of 0.350 M Ba(OH), was added to 55.0 mL of 0.700 M HCI. The reaction caused the temperature of the solution to rise from 23.81 °C to 28.58 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g °C.) respectively), what is AH for this reaction (per mole H₂O produced)? Assume that the total volume is the sum of the individual volumes. AH= kJ/mol H₂Oarrow_forwardIn the following reaction, how much heat is generated when 3.21 moles of CH4 are burned? CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O(g) AH° = -802 kJ/molarrow_forwardA chemist measures the energy change AH during the following reaction: 2 H₂O(l) → 2 H₂(g) + O₂(g) ΔΗ= 572. kJ Use the information to answer the following questions. This reaction is... Suppose 64.5 g of H₂O react. Will any heat be released or absorbed? If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Round your answer to 3 significant digits. O endothermic. O exothermic. O Yes, absorbed. O Yes, released. O No. 0 kJ x10 Start overarrow_forward
- A 5.71 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 °C. After the salt has completely dissolved, the temperature of the solution is 28.54 °C. What quantity in moles of the unknown salt were used in the reaction?arrow_forwardDetermine the amount of heat released when 180.00 g AsBr5(g) reacts according to the following equation: As4O10(g) + 6 AsBr5(g) → 10 Br3AsO(g) Additional equations that may be useful: 1/4 As4(s) + 3/2 Br2(g) → AsBr3(g) ΔH = -336.4 kJ/mol As4(s) + 5 O2(g) → As4O10(g) ΔH = -2967.3 kJ/mol AsBr3(g) + Br2(g) → AsBr5(g) ΔH = -84.2 kJ/mol AsBr3(g) + 1/2 O2(g) → Br3AsO(g) ΔH = -295.7 kJ/molarrow_forwardConsider the following reaction: 2Mg(s)+O2(g)⟶2MgO(s)ΔH∘=−1203kJ What mass of magnesium must be combusted in order to generate 174.0 kJ of heat?arrow_forward
- When 3.8 g A are reacted with 8.5 g D, according to the balanced chemical equation below, 33 kJ of energy are released. Please calculate the enthalpy for this reaction when 3 moles of G are produced. 2A + 3D = 2Z + 3G given molar masses: A = 141.8 g/mole D = 63.996 g/ mole Z = 4.032 g/ mole G = 56.028 g/ molearrow_forward8. Instant cold packs can be made from ammonium nitrate by mixing/reacting it with water (reaction shown below). When 1.25 g of NH4NO3 is dissolved in 25.0 g of water at 25.8 °C, the temperature of the water after the reaction is 21.9 °C. What is the enthalpy change (ΔH) for this reaction in units of kJ/mol of NH4NO3? The heat capacity of water is 4.18 ?/ ?℃ . NH4NO3(s) → NH4+(aq) + ??3 − (aq)arrow_forwardIn a calorimeter, a 2.0 g sample of magnesium is burned to form MgO. In doing so, 25.5 kJ of energy are released. What is the Heat of Combustion in kJ/mol of magnesium? с 306.2 1.54 x 1025 0.0392 514 25.5arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY