increases4. In a coffee-cup calorimeter, 50.0 mL of 0.100 M AgNO3 at 22.6°C are mixed with 50.0 mL of 0.100 M HCI) also at22.6°C. The final temperature of the resulting solution is 27.9°C. The final solution has a combined mass of 100.0grams and a specific heat capacity of 4.18 J/g°C.2) HC (9) Ag! (b)Ag +→ AgCl(s) + HNO3 (99)⑨Ag NO HCAgt CH NO H+ / No Ag + C1→ AgCla. Write a balanced equation for this reaction.b. Write the net ionic equation for this reaction.b. How many moles of solid product are formed? | molNO3THI(clic. Calculate the enthalpy change that accompanies this reaction (AH) in kJ/mole of solid product.d. Is this reaction exothermic or endothermic? How do you know?

As per the guidelines, only first 3 subparts will be answered.a.Given: AgNO3 mixed with HClBalanced…

Creases 4. In a coffee-cup calorimeter, 50.0 mL of 0.100 M AgNO3 at 22.6°C are mixed with 50.0 mL of 0.100 M HCI) also at 22.6°C. The final temperature of the resulting solution is 27.9°C. The final solution has a combined mass of 100.0 grams and a specific heat capacity of 4.18 J/g°C. AgNO HC lags Ag(s)+ HNO3 (99) Agl NO, Ag + CI→ AgCl a. Write a balanced equation for this reaction. b. Write the net ionic equation for this reaction. b. How many moles of solid product are formed? I mol AgCH NOH HT (cli c. Calculate the enthalpy change that accompanies this reaction (AH) in kJ/mole of solid product. d Is this reaction eve

Creases 4. In a coffee-cup calorimeter, 50.0 mL of 0.100 M AgNO3 at 22.6°C are mixed with 50.0 mL of 0.100 M HCI) also at 22.6°C. The final temperature of the resulting solution is 27.9°C. The final solution has a combined mass of 100.0 grams and a specific heat capacity of 4.18 J/g°C. AgNO HC lags Ag(s)+ HNO3 (99) Agl NO, Ag + CI→ AgCl a. Write a balanced equation for this reaction. b. Write the net ionic equation for this reaction. b. How many moles of solid product are formed? I mol AgCH NOH HT (cli c. Calculate the enthalpy change that accompanies this reaction (AH) in kJ/mole of solid product. d Is this reaction eve

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 60E: In a coffee-cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCI are mixed. Both...

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Consider the reaction 2HCl(aq)+Ba(OH)2(aq)BaCl2(aq)+2H2O(l)H=118KJ Calculate the heat when 100.0 rnL of 0.500 M HCl is mixed with 300.0 mL of 0.100 M Ba(OH)2 Assuming that the temperature of both solutions was initially 25.0C and that the final mixture has a mass of 400.0 g and a specific heat capacity of 4.18 J/C g, calculate the final temperature of the mixture.
A student performing a calorimetry experiment combined 100.0 ml. of 0.50 M HCI and 100.0 ml. of 0.50 M NaOH in a StyrofoamTM cup calorimeter. Both solutions were initially at 20.0 C, but when the two were mixed, the temperature rose to 23.2 C (a) Suppose the experiment is repeated in the same calorimeter but this time using 200 mL of 0.50 M HCl and 200.0 ml of 0.50 M NaOH. WIII the AT observed be greater than, less than, or equal to that in the first experiment, and why? (b) Suppose that the experiment is repeated once again in the same calorimeter, this time using 100 mL of 1.00 M HCI and 100.0 ml. of 1.00 M NaOH. Will the T observed be greater than, less than, or equal to that in the first experiment, and why?
When 1.0 g of fructose, C6H12O6(s), a sugar commonly found in fruits, is burned in oxygen in a bomb calorimeter, the temperature of the calorimeter increases by 1.58 C. If the heat capacity of the calorimeter and its contents is 9.90 kJ/C, what is q for this combustion?
A sample of benzene, C6H6, weighing 3.51 g was burned in an excess of oxygen in a bomb calorimeter. The temperature of the calorimeter rose from 25.00C to 37.18C. If the heat capacity of the calorimeter and contents was 12.05 kJ/C, what is the value of q for burning 1.00 mol of benzene at constant volume and 25.00C? The reaction is C6H6(l)+152O2(g)6CO2(g)+3H2O(l) Is q equal to U or H?
A sample of ethanol, C2H5OH, weighing 2.84 g was burned in an excess of oxygen in a bomb calorimeter. The temperature of the calorimeter rose from 25.00C to 33.73C. If the heat capacity of the calorimeter and contents was 9.63 kJ/C, what is the value of q for burning 1.00 mol of ethanol at constant volume and 25.00C? The reaction is C2H5OH(l)+3O2(g)2CO2(g)+3H2O(l) Is q equal to U or H?
When 50.0 g of 0.200 M NaCl(aq) at 24.1 C is added to 100.0 g of 0.100 M AgNO3(aq) at 24.1 C in a calorimeter, the temperature increases to 25.2 C as AgCl(s) forms. Assuming the specific heat of the solution and products is 4.20 J/g C, calculate the approximate amount of heat in joules produced.
Ammonium nitrate is an oxidizing agent and can give rise to explosive mixtures. A mixture of 2.00 mol of powdered aluminum and 3.00 mol of ammonium nitrate crystals reacts exothermically yielding nitrogen gas, water vapor, and aluminum oxide. How many grams of the mixture are required to provide 245 kJ of heat? See Appendix C for data.
In a coffee-cup calorimeter, 150.0 mL of 0.50 M HCI is added to 50.0 mL of 1.00 M NaOH to make 200.0 g solution at an initial temperature of 48.2C. If the enthalpy of neutralization for the reaction between a strong acid and a strong base is 56 kJ/mol, calculate the final temperature of the calorimeter contents. Assume the specific heat capacity of the solution is 4.184 J/g C and assume no heat Joss to the surroundings.
A 250-g sample of water at 20.0C is placed in a freezer that is held at a constant temperature of 20.0C. Considering the water as the system, answer the following questions: a What is the sign of qsys for the water after it is placed in the freezer? b After a few hours, what will be the state of the water? c How will the initial enthalpy for the water compare with the final enthalpy of the water after it has spent several hours in the freezer? d What will the temperature of the water be after several hours in the freezer?
A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g water at 23.5C. After the metal cools, the final temperature of metal and water mixture is 25.0C. If the specific heat capacity of nickel is 0.444 J/C g, what mass of nickel was originally heated? Assume no heat loss to the surroundings.
A 50-mL solution of a dilute AgNO3 solution is added to 100 mL of a base solution in a coffee-cup calorimeter. As Ag2O(s) precipitates, the temperature of the solution increases from 23.78 C to 25.19 C. Assuming that the mixture has the same specific heat as water and a mass of 150 g, calculate the heat q. Is the precipitation reaction exothermic or endothermic?

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