The following reaction using hydrogen and oxygen is carried out in a bomb calorimeter: 2H2(9) + O2(g) → 2H2O() The specific heat of the reaction vessel is 0.200 kcal/°C-kg and the specific heat of water is 1.00 kcal/°C-kg. Assuming that m is 0.2 mole of water was formed in the experiment and Q is 3.7 kcal, calculate the heat of the reaction per mole of liquid water.

The following reaction using hydrogen and oxygen is carried out in a bomb calorimeter: 2H2(9) + O2(g) → 2H2O() The specific heat of the reaction vessel is 0.200 kcal/°C-kg and the specific heat of water is 1.00 kcal/°C-kg. Assuming that m is 0.2 mole of water was formed in the experiment and Q is 3.7 kcal, calculate the heat of the reaction per mole of liquid water.

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

Measurements show that the energy of a mixture of gaseous reactants decreases by 178. kJ during certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that -163. kJ of work is done on the mixture during the reaction. Calculate the change in enthalpy of the gas mixture during the reaction. Round your answer to 2 significant digits. Is the reaction exothermic or endothermic? kJ exothermic endothermic x10 X
Measurements show that the enthalpy of a mixture of gaseous reactants decreases by 323. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that -162. kJ of work is done on the mixture during the reaction. Calculate the change in energy of the gas mixture during the reaction. Round your answer to 3 significant digits. Is the reaction exothermic or endothermic? kJ exothermic O endothermic x10 X 3
You place 32.3 ml of 0.134 M Ba(OH), in a coffee-cup calorimeter at 25.00°C and add 60.6 ml of 0.433 M HCI, also at 25.00°C. After stirring, the final temperature is 28.63°C. {assume that the total volume is the sum of the individual volumes and that the final solution has the same density (1.00 g/ml) and specific heat capacity (4.184 J/g°C) as water}. Calculate the change in enthalpy, AH, of the reaction (in kJ/mol) of water formed. Enter the appropriate sign (+/-). Enter a number to 1 decimal place.
Consider the combustion of liquid CsHs in oxygen gas to produce carbon dioxide gas and water vapor. In an experiment, 0.1063 g of CsHs is combusted to produce enough heat to raise the temperature of 150.0 g of water by 7.632 °C. If -4790 J of heat was produced from the combustion of 0.001561 moles of CsHs, what is the enthalpy change (in kJ/mol) for the combustion of CsHs?
In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.00 mL of 1.00 M HCl are mixed. Both solutions were originally at 24.6 C. After the reaction, the final temperature is 31.3 C. Given that the density of NaCl solution is 1.038 g/mL and the specific heat of NaCl solution is 3.87, calculate the change in enthalpy of neutralization per mole for the reaction of HCl with NaOH. Assume that no heat is lost to the surroundings.
Calculate the standard enthalpy for the reaction: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g), given the following data: N2(g) + O2(g) → 2NO(g) ΔHrxn = -43.1 kcal mol-1 N2(g) + 3H2(g) → 2NH3(g) ΔHrxn = -21.9 kcal mol-1 2H2(g) + O2(g) → 2H2O(g) ΔHrxn = -115.6 kcal mol-1
Consider these reactions: Reaction 1: H₂(g) + Cl₂(g) → 2HCl(g) AH-184.6 kJ Reaction 2:20F₂(g) → O₂(g) + 2 F2 (9) AH-49.4 kJ Reaction 3: N₂(g) +202 (9) 2NO₂(g) AH = +66.4 kJ Use Reaction 2. → How much energy (in kJ) is released when 73.0 g of oxygen difluoride decomposes? Answer: - kJ (enter a positive value)
9
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?
Calculate the standard enthalpy for the reaction: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g), given the following data: N2(g) + O2(g) → 2NO(g) ΔHrxn = -43.1 kcal mol-1 N2(g) + 3H2(g) → 2NH3(g) ΔHrxn = -21.9 kcal mol-1 2H2(g) + O2(g) → 2H2O(g) ΔHrxn = -115.6 kcal mol-1 Round your answer to 2 decimal places.
Calculate AH for the reaction P4010(s) + 6PC15(g) – 10C13PO(g) given, P4(s) + 6C12(g) → 4PC13(g) AH = -1225.6 kJ P4(s) + 502(g) – P4010(s) AH = -2967.3 kJ PC13(g) + Cl2(g) → PC15(g) AH = -84.2 kJ PC13(g) + (1/2)02(g) – C13PO(g) AH=-285.7 kJ ΔΗ- kJ
5.00 × 10−2 mol KOH and an excess of hydrochloric acid are combined in 100.0 mL of water initially at 25.0 °C, leading to a final measured temperature of 31.1 °C. (a) What is the heat flow for the water in the calorimeter, qH2O, in Joules? (b) Assuming the calorimeter constant Ccal = 50.0 J °C , what is the heat flow for the calorimeter, qcal, in Joules? (c) What is the amount of heat given off by the reaction, qrxn, in Joules? (d) What is the molar enthalpy of the neutralization reaction (shown below) as measured in the calorimeter, ∆H◦ rxn in kilojoules per mole? H3O + (aq) + OH– (aq) → 2H2O (l)