Tutored Practice Problem 10.4.5 COUNTS TOWARDS GRADEClose ProblemUse constant-volume calorimetry to determine energy change.A 0.527-g sample of benzoic acid (C,H,02) is burned in a bomb calorimeter and the temperature increasesfrom 24.80 °C to 27.50 °C. The calorimeter contains 1.10x10 g of water and the bomb has a heat capacity of814 J/°C. Based on this experiment, calculate AE for the combustion reaction per mole of benzoic acidburned (kJ/mol).C,H,O2(s) + 15/2 O,®) 7 CO,(g) + 3 H,0(1) AEkJ/molThe reaction of carbon monoxide(g) with nitrogen monoxide(g) to form carbondioxide(g) and nitrogen(g) proceeds as follows:2 CO(g) + 2 NO(g) →2 CO2(g) + N2g)When 8.54 grams of CO(g) react with sufficient NO(g) , 114 kJ of energy areevolved.What is the value of AH for the chemical equation given?AHn = 373.90kJrxnThe following thermochemical equation is for the reaction of hydrogenchloride(g)with ammonia(g) to form ammonium chloride(s).HCI(g) + NH3(g)→ NH¾CI(s) AHxn=-176 kJHow many grams of HCl(g) would have to react to produce 63.0 kJ of energy?grams

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A 0.527-g sample of benzoic acid (C,H,0,) is burned in a bomb calorimeter and the temperature increases from 24.80 °C to 27.50 °C. The calorimeter contains 1.10x10 g of water and the bomb has a heat capacity of 814 JrC. Based on this experiment, calculate AE for the combustion reaction per mole of benzoic acid burned (kJ/mol). C,HO2(s) + 15/2 O,(g)- →7 CO2(g) + 3 H,OI) |kJ/mol AE -

A 0.527-g sample of benzoic acid (C,H,0,) is burned in a bomb calorimeter and the temperature increases from 24.80 °C to 27.50 °C. The calorimeter contains 1.10x10 g of water and the bomb has a heat capacity of 814 JrC. Based on this experiment, calculate AE for the combustion reaction per mole of benzoic acid burned (kJ/mol). C,HO2(s) + 15/2 O,(g)- →7 CO2(g) + 3 H,OI) |kJ/mol AE -

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...

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A 6.78 g sample of methanol was combusted in a bomb calorimeter. The temperature of the calorimeter increased by 12.7 °C. If the molar mass of methanol is 32.04 g/mol, and the heat capacity of the calorimeter is 5,104 J/°C, what is the molar AE for this reaction, in kJ/mol? Do not report units in your answer. Report your answer to one decimal place and include the correct sign.
When 1.836 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?
pt pt pt pt pt pt pt pt pt pt pt pt pt pt You should use care when dissolving H₂SO4 in water because the process is highly exothermic. To measure the enthalpy change, 5.8 g of concentrated H₂SO4() was added (with stirring) to 140. g of water in a coffee-cup calorimeter. This resulted in an increase in temperature from 21.0 °C to 30.3 °C. Calculate the enthalpy change for the process H₂SO4(l) → H₂SO4 (aq), in kJ/mol. Assume the specific heat capacity of the solution is 4.2 J/g. K. Enthalpy change = kJ/mol ?
The complete combustion of salicylic acid releases 21.90 kJ of energy per gram of salicylic acid.In a particular bomb calorimeter (initially at room temperature), the combustion of 0.2745 g of salicylic acid, in the presence of excess oxygen, causes the temperature of the calorimeter to rise by 1.85 °C.When a 0.2999-g sample of an unknown organic substance is similarly burned in the same calorimeter, the temperature rises by 3.59 °C.What is the energy of combustion per unit mass of the unknown substance?
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When 9.1 g of a hydrocarbon is combusted in a bomb calorimeter the temperature of the calorimeter increases from 23.8 C to 53.5 C. The calorimeter contains 731 g of water and the heat capacity of the bomb is 872 J/ C. Please calculate q rxn, in kJ, for the combustion of the hydrocarbon.
At constant volume, the heat of combustion of a particular compound, compound A, is −3046.0 kJ/mol.−3046.0 kJ/mol. When 1.753 g1.753 g of compound A (molar mass =112.07 g/mol)=112.07 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 6.475 ∘C.6.475 ∘C. What is the heat capacity (calorimeter constant) of the calorimeter? Suppose a 3.771 g3.771 g sample of a second compound, compound B, is combusted in the same calorimeter, and the temperature rises from 25.65 ∘C25.65 ∘C to 29.76 ∘C.29.76 ∘C. What is the heat of combustion per gram of compound B?
2. Consider the equation for the combustion of acetone (C₁H₂O), the main ingredient in nail polish remover. AHR -1790 kJ CHO (l)+4Oz (g) -> 3 CO, (g)+3H,O (g) If a bottle of nail polish remover contains 255 g of acetone, how much heat is released by its complete combustion?
A 3.000 g sample of food was then burned in a calorimeter to determine its Calories per gram content. 50mL of water were used to determine ΔT of the reaction. Initial temperature of the water at the start of the combustion reaction was 20oC, final temperature was 99oC. Calorimeter constant for this calorimeter is 10.0J/oC. How much heat has been absorbed by the water sample?
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THERMODYNAMICS: A 1.96 g sample of acetic acid (HC;H3O2) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/°C, contained 776 g of water. The temperature of the calorimeter and its contents increased from 24.51°C to 27.95°C. What is AH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 g/mol. (Round off the final answer to ONE decimal place) Round your answer to 1 decimal place.