Heat Evolved (J)5045403530201510SRelationship Between Amount of Reactant and Energy°1020507090100Males of Reactant (mol)Use the graph above to determine how much heat energy, in Joules, would be evolved by reacting 90.0 mol of reactant. Enter a numerical value in the box provided; do not enter units.Type answer:

Answered: Image /qna-images/answer/53df16a9-3e47-47c4-93f5-7b91542bdeaa.jpg

Answered: Heat Evolved (J) 50 45 40 35 30 20 15…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

13. Determine the amount of heat (in kJ) given off when 320 g of NO, are produced according to the equation: 2 NO(g) + 0,(g) 2 NO,(g) ΔΗ - -114.6 kJ/mol (Molar mass of NO, = 46 g/mol) * -1.49 x 10+2 -6.48 x 10+2 -3.99 x 10+2 O -2.74 x 10*2 -5.23 x 10+2 If th
A calorimeter is an insulated device in which a chemical reaction is contained. By measuring the temperature change, AT, we can calculate the heat released or absorbed during the reaction using the following equation: Constants Periodic Table Part A q = specific heat x mass x AT A calorimeter contains 30.0 mL of water at 14.0 °C. When 1.70 g of X (a substance with a molar mass of 76.0 g/mol ) is added, it dissolves via the reaction Or, if the calorimeter has a predetermined heat capacity, C, the equation becomes X(s) + H2O(1)→X(aq) q=C x AT and the temperature of the sblution increases to 30.0 °C At constant pressure, the enthalpy change for the reaction, AH, is equal to the heat, qp; that is, Calculate the enthalpy change, AH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water (4.18 J/(g. °C)J, that density of water is 1.00 g/mL, and that no heat is lost to the calorimeter itself, nor to the suroundings. ΔΗp Express the…
3. During the experiment, when calculating AH using the formula AH=C x AT, can we calculate the AH without measuring the amount of water that we put inside the calorimeter? Explain why or why not. (max of 5 sentences) 4. You accidentally forgot to measure the mass of the octane that you transferred in the crucible. You already started the calorimeter and it is too late to stop the equipment. Is it still possible to calculate the energy (in Joules) of octane? Explain.(max of 2 sentences)
3
Please help me complete this question
In an exothermic chemical reaction O heat is released as the reaction proceeds. the mass of the products is greater than the mass of the reactants. the mass of the products is less than the mass of the reactants. O heat is absorbed as the reaction proceeds.
2. A student collect experimental results and show all calculation steps including units. Keep the correet significant figures. Part 1: Calculation of the calorimeter constant (15 pts) Mass of Mass of Temperature of cold water in calorimeter cold water hot water Temperature of hot water before mixing 57.3°C Final temperature of the water after mixing 36.8°C 61.0 g 56.2 g 22.6 °C Show calculations below. Part II: Conduct Reaction 1 between solutions of NaOH and HCI (20 pts) Volume of Volume of Density of the NaOH HCI Initial temperature of the solution in the calorimeter solution solution. solution 51.0 mL 52.0 mL 1.04 g/mL 22.6 °C Show calculations below. Final temperature of the reaction mixture 32.2 °C The calorimeter constant is: Enthalpy of the reaction, in kJ/mol, is
A chunk of gold (specific heat: 0.126) initially at 82.2 ˚C is placed in 75.5 g of water (specific heat: 184) initially at 22.0 ˚C. After a short time, both the water and the gold are at 41.0 ˚C. What was the mass of the gold?
1
What are some examples of exothermic and endothermic reactions or processes you've seen in real life aside from hot and cold packs?
In order to break water into hydrogen and oxygen, water is heated to more than 500°C. Which kind of reaction is this and why? It is exothermic because heat needs to be released by the reactants to form the products. It is endothermic because heat needs to be released by the reactants to form the products It is exothermic because heat needs to be absorbed by the reactants to form the products. It is endothermic because heat needs to be absorbed by the reactants to form the products.
Specific heat is the heat required to raise the temperature of 1 g of a substance by 1 °C. Based on this definition, what is the equation to calculate specific heat? Select one: heat O specific heat = %3D (mass x temperature change) temperature change specific heat = mass (heat x tempetature change) specific heat = mass temperature change O specific heat = (mass x heat)

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

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

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

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

SEE MORE TEXTBOOKS