A 104.4mL sample of 1.8M HNO3 is mixed with a 800mL sample of 0.5M KOH in a Styrofoam cup. If bothsolutions were initially at 25.2\deg C, and the enthalpy of the neutralization reaction is -57 kJ/mole of H2Oformed, what is the final temperature of the mixture? The volume of the formed H2O can be ignored. Assumethat the solution has a density of 1.00 g/mL and a specific heat of 4.184 J/g\deg C, and that the Styrofoamcup has an insignificant heat capacity. (enter one decimal place)

THE FINAL TEMPERATURE OF THE MIXTURE IS 25.98 0CExplanation:Approach to solving the quest

Answered: A 104.4mL sample of 1.8M HNO3 is mixed…

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

The lead-acid storage battery is the oldest rechargeable battery in existence. It was invented in 1859 by French physician Gaston Plante and still retains application today, more than 150 years later. There are two reactions that take place during discharge of the lead-acid storage battery. In one step, sulfuric acid decomposes to form sulfur trioxide and water: H2SO4(l) →SO3(g) +H2O(l) =ΔH+113.kJ In another step, lead, lead(IV) oxide, and sulfur trioxide react to form lead(II) sulfate: Pb(s) +PbO2(s) +2SO3(g) →2PbSO4(s) =ΔH−775.kJ Calculate the net change in enthalpy for the formation of one mole of lead(II) sulfate from lead, lead(IV) oxide, and sulfuric acid from these reactions.Round your answer to the nearest kJ.
For the reaction 4HCI(g) + O₂(g)—2H₂O(g) + 2Cl₂(g) AH° = -114.4 kJ and AS° = -128.9 J/K The maximum amount of work that could be done when 2.34 moles of HCI(g) react at 255 K, 1 atm is Assume that AH° and AS° are independent of temperature. kJ.
A glass is filled to the brim with 480.0 mL of water at 100.0 ∘C. If the temperature of glass and water is decreased to 20.0 ∘C, how much water could be added to the glass?
Solid potassium fluoride is dissolved in water in a perfect calorimeter. When 10.00 grams of potassium fluoride is dissolved in 120.0 grams of water initially at a temperature of 20.00 °C, the temperature of the solution increases to 25.61 °C. Calculate AHⓇ for the reaction below in kJ/mol. KF (s) → K+ (aq) + F¯¯ (aq) AH°= ? [You may assume that no heat escapes the calorimeter and that all solutions have the same specific heat capacity as pure water (4.184 J/g °C)] • Was energy released by the salt into the water or was energy absorbed by the salt from the water? Think about how the temperature of the water changed. What does this tell you about AH for the reaction taking place? Is the process of dissolving the salt endothermic or exothermic? What is the sign of AH? ΔΗ= positive (Remember this!) Energy does not escape the calorimeter. So, if energy is released by the reaction it must be take into (absorbed) by the water. If energy is absorbed by the reaction, it must have been taken…
What is the theory of the first law of thermodynamics ?
I need help answering 4a.
Consider the following reaction at 25 °C: 3 NiO(s) + 2 NH3(g) → 3 Ni(s) + N2(g) + 3 H20(g) If AG° = -18.1 kJ/mol, determine the value of AG assuming that a mixture contains 57.6 g of NiO, 182.3 g of Ni, 0.24 atm of NH3, 8.54 atm of N2 and 10.07 atm of H2O. kJ 1 2 3 4 6. C 7 8 9. +/- х 100 +
Reactions between acids and bases (neutralization reactions) are exothermic. You have a solution of an acid and a solution of a base, both at 23oC. If you mix the two solutions together, would you expect the final temperature to be greater or less than 23oC?
i (1 L atm = 101.325 J, 1 L bar = 100.000 J) The oxidation of nitric oxide 2 NO(g) + O2(g) → 2 NO2(g) AH =-113.1 kJ is a key step in the production of photochemical smog. Calculate the change in internal energy (in kJ) that occurs when 250.0 g of NO reacts with excess oxygen at 85.0°C.
For the reaction 2 C6H5COOH(s) + 15 O₂(g) →14 CO₂(g) AUrxn = -772.7 kJ/mol at 298K. Calculate AHrxn. + 6 H₂O(g)
mmetal 15.740 Next, heat up the piece of iron and record the metal's highest temperature, Tmetal · Tmetal =| 53.30 Enter numeric value Next, record the mass of water (mwater) in the coffee cup. mwater 60.0 Record the initial temperature of the water, Twater1, in the coffee cup. Twaterl 25 Place the hot piece of iron into the cool water and record the final temperature of the water, Twater2.
Two solutions, initially at 24.60°C, are mixed in a coffee cup calorimeter. When a 100.0 mL volume of 0.100 M AgNO3 solution is mixed with a 100.0 mL sample of 0.200 M NaCl solution, the temperature in the calorimeter rises to 25.30°C. Determine the ΔH°rxn for the reaction as written below. Assume that the density and heat capacity of the solutions is the same as that of water. The specific heat capacity of water = 4.18 J/g°C.NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) ΔH°rxn = ?

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