enriched to a 60 wt % sulfuric acid solution by adding pure sulfuric acid. a. How much pure sulfuric acid should be added? b. If the 20 wt % solution is available at 5°C, and the pure sulfuric acid at 50°C, how much heat will have to be removed to produce the 60 wt % solu- tion at 70°C? How much heat will have to be added or removed to produce the 60 wt% solution at its boiling point?

enriched to a 60 wt % sulfuric acid solution by adding pure sulfuric acid. a. How much pure sulfuric acid should be added? b. If the 20 wt % solution is available at 5°C, and the pure sulfuric acid at 50°C, how much heat will have to be removed to produce the 60 wt % solu- tion at 70°C? How much heat will have to be added or removed to produce the 60 wt% solution at its boiling point?

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 52E: Before the introduction of chlorofluorocarbons, sulfur dioxide (enthalpy of vaporization, 6.00...

See similar textbooks

Similar questions

The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)
When one mol of KOH is neutralized by sulfuric acid, q=56 kJ. (This is called the heat of neutralization.) At 23.7C, 25.0 mL of 0.475 M H2SO4 is neutralized by 0.613 M KOH in a coffee-cup calorimeter. Assume that the specific heat of all solutions is 4.18J/gC, that the density of all solutions is 1.00 g/mL, and that volumes are additive. (a) How many mL of KOH is required to neutralize H2SO4? (b) What is the final temperature of the solution?
Find the heat of reaction and explain what happen to it. Calculate the ∆H of reaction for: C3H8 (g) + 5O2 (g) => 3CO2 (g) + 4H2O (l) The values of ∆H of reaction are as follows:C3H8 (g) = -103.95 kJ/molCO2 (g) = -393.5 kJ/molH2O (g) = -285.8 kJ/mol Topic: Enthalpy of Reaction
Calculate delta H of formation for the compound Ni2O3, given the following: Ni(s) + 1 1/2 O2(g) ----> Ni2O3(s) Mass of Calorimeter: 6000 g SP of calorimeter: 0.44 j/g*c Mass of water: 12000 g SP of water: 4.18 j/g*c #g of Ni used 19.33g #g of O2 used 21.3g Initial water temp: 21.45*c Final water temp: 24.63*c
For items 1-3, refer to the equation: CH4(g) + 2O2(g) → 2H2O(l) + CO2(g), with ΔH equal to -809.94 kJ/mol.1. Is the reaction heat-producing (exothermic) or heat-absorbing(endothermic)?2. How many moles of liquid water (H2O(l)) will be produced upon combustion of 3 moles of methane gas (CH4(g))?3. Calculate the ΔH if 5g of methane gas was combusted. With solutions and explanation.
For items 1-3, refer to the equation: CH4(g) + 2O2(g) → 2H2O(l) + CO2(g), with ΔH equal to -809.94 kJ/mol.1. Is the reaction heat-producing (exothermic) or heat-absorbing(endothermic)?2. How many moles of liquid water (H2O(l)) will be produced upon combustion of 3 moles of methane gas (CH4(g))?3. Calculate the ΔH if 5g of methane gas was combusted.For the following items, choose the letter of the correct answer. Write it on your answer sheet in ALL UPPERCASE letters. 4. A process in which there is no thermal energy exchanged between a system and its surroundings is called a/an:a. isothermal process b. isobaric processc. diathermic process d. adiabatic process5. According to Hess’ Law, the amount of energy expenditure for the same end-product will vary dependent on the number of steps.a. Statement above is true.b. Statement above is incorrect.c. Statement above is indeterminate.d. Statement above lacks varied data to make a judgement. Please answer all the questions.
A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 68.5 mL water (where X is a hypothetical metal): X + 2 HCI ---> XCI2 + H2 In this process, the water temperature rose from 25.0 °C to 33.3 °C. If 0.00629 mol of "X" was consumed during the reaction, what is ?rH of this reaction in kJ mol^-1with respect to "X"? The specific heat of water is 4.184 J g-¹ °C-¹
At constant pressure and 25℃, what is ∆H° for the following reaction 2C2H6 (g)+7O2 (g)→4CO2 (g)+H2O(l) If the complete consumption of 38.2g of C2H6 liberates 1981 kJ of heat energy?
A group of Chemistry students was asked to determine the heat of reaction forthe neutralization of a newly synthesized monoprotic acid HX and NaOH. Theyfirst calibrated the styro ball calorimeter using the reaction of 15.0 mL of 0.100 MHCl and 20.0 mL of 0.0500 M KOH. This recorded a change in temperature from26.5 °C to 31.8 °C. Afterwards, they determined the heat of reaction for a mixtureof 5.00 mL, 1.00 M NaOH and 10.0 mL, 1.00 M HX. This showed an increase intemperature of 3.6 °C. What is the heat capacity of the calorimeter in J/℃ (∆??????????????? =-55.85kJ/mol)?
Students were asked to determine the heat of reaction forthe neutralization of a newly synthesized monoprotic acid HX and NaOH. Theyfirst calibrated the styro ball calorimeter using the reaction of 15.0 mL of 0.100 MHCl and 20.0 mL of 0.0500 M KOH. This recorded a change in temperature from26.5 °C to 31.8 °C. Afterwards, they determined the heat of reaction for a mixtureof 5.00 mL, 1.00 M NaOH and 10.0 mL, 1.00 M HX. This showed an increase intemperature of 3.6 °C.i. What is the heat capacity of the calorimeter in J/℃ (∆? =-55.85??????????????kJ/mol)?ii. Write the balanced chemical and net ionic equations for the reaction of NaOHand HX .iii. What is the experimental enthalpy (in kJ/mol) for the neutralization reactionbetween HX and NaOH ?iv. Is the reaction between NaOH and HX endothermic or exothermic ?
Write a balanced equation for the combustion of CH3C6H13(l) (methyl hexane)-- i.e. its reaction with O2(g) forming the products CO2(g) and H2O(l). Given the following standard heats of formation: ΔHf° of CO2(g) is -393.5 kJ/mol ΔHf° of H2O(l) is -286 kJ/mol ΔHf° of CH3C6H13(l) is -173.0 kJ/mol What is the standard heat of reaction (ΔH°) for the combustion reaction of CH3C6H13(l)? Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of methyl hexane. (Assume standard state conditions and 298 K for all reactants and products.)
Using the following data of heats of combustion in cal/g mole, calculate thefollowing:(a) Heat of vaporization of benzene – cal/g mole(b) Heat of combustion of benzene to wateri) C6H6 (l) → CO2 (g) and H2O (l) = 780,980ii) C6H6 (g) → CO2 (g) and H2O (g) = 759,520iii) H2 (g) → H2O (l) = 68,317iv) H2 (g) → H2O (g) = 59,798v) Graphite to CO2 (g) = 94,052