4 moles of A, (g) reacts completely with 2 moles of B, (g) to form 4 moles of A,B (g) in a corstant volume container at 30 °C. The heat released from this reaction increased the temperature of 50g water by 5 C. Calculate the enthalpy change of the reaction per mole consumption of B, (g). Specific heat capacity of water, c = 4.184 J g K-1 R = 0.08206 L atm mol-1 K-1 = 8.314 J mo1-1 K-1

4 moles of A, (g) reacts completely with 2 moles of B, (g) to form 4 moles of A,B (g) in a corstant volume container at 30 °C. The heat released from this reaction increased the temperature of 50g water by 5 C. Calculate the enthalpy change of the reaction per mole consumption of B, (g). Specific heat capacity of water, c = 4.184 J g K-1 R = 0.08206 L atm mol-1 K-1 = 8.314 J mo1-1 K-1

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

A 100.0 mL sample of 0.250 M NaOH is mixed with a 150.0 mL sample of 0.280 M HNO3 in a coffee cup calorimeter. Both solutions were initially at 35.00°C and after mixing, the temperature of the resulting solution was recorded as 37.00°C. Determine the enthalpy of neutralization (ΔH°neutralization rxn) (in units of kJ/mol) for the neutralization reaction between aqueous NaOH and HNO3. The specific heat capacity of water = 4.184 J/g°C and density of water = 1.00 g/mL Assume 1) that no heat is lost to the calorimeter or the surroundings, and 2) that the density and the heat capacity of the resulting solution are the same as water. Hint: Heat of neutralization is the enthalpy change per mol of water formed in a neutralization reaction. Write the balanced equation, calculate the limiting reactant and the mol of water formed in the reaction. Enter the numerical value clearly indicating whether it is endothermic or exothermic.
is this the standard enthalpy change, enthalpy change, enthalpy of solution, or the standard molar enthalpy of formation?
2. Determine the standard enthalpy change (AH°) for the reaction: C,H6 le) + 7/2 Ozle) 2CO2le) + 3H,0»
The overall reaction in a commercial heat pack can be represented as 4 Fe(s) +302 (9)2 Fe, O, (s) AH=-1652 kJ a. How much heat is released when 4.00 moles of iron are reacted with excess O2? Heat = kJ b. How much heat is released when 1.00 mole of Fe2O3 is produced? Heat = kJ c. How much heat is released when 1.40 g iron is reacted with excess 02? Heat kJ %3D d. How much heat is released when 10.8 g Fe and 1.50 g O2 are reacted? Heat kJ
The thermite reaction, used for welding iron, is the reaction of Fe3O4 with Al. 8 Al (s) + 3 FezO4 (s) > 4 Al203 (s) + 9 Fe (s) AH° = -3350 kJ Because this large amount of heat cannot be rapidly dissipated to the surroundings, the reacting mass may reach temperatures near 3000°C. How much heat (in kJ) is released by the reaction of 14.7 g of Al with 63.1 g of Fe3O4? Enter your numerical answer in units of kJ.
6. 100.0 mL of 1.00 M of HCl and 100.0 mL of 2.00 M of Ca(OH)2 are mixed at 298K. During the experiment, the temperature rose to 298.0067 K. Assume the heat capacities of the two solutions and densities are the same as that of water (4.184 J/g °C and 1.00 g/mL). Calculate the heat of neutralization in units of (kJ/mol H₂0 produced).
Use the following information to calculate the standard enthalpy of formation of NO>(g) at 298 K? N2(g)+ O2(g) - 2NO(g) AH =180.5 kJ 298 NO2(g) - % O2(g) + NO(g) AHOR =57.06 kJ
Part C Consider the exothermic reaction C3H$ (g) + 100, (g)→3CO2 (g) + 4H2O(g) Calculate the standard heat of reaction, or AH°, for this reaction using the given data. Also consider that the standard enthalpy of the formation of elements in their pure form is considered to be zero. Reactant or product Af H° (kJ mol 1) C,Hs(9) -104 CO2(9) -393.5 H2O(g) -241.8 Express your answer to four significant figures and include the appropriate units. • View Available Hint(s) HA Value Units
For the reaction N2(g) + 3H2(g) →2NH3(g) AG° = -29.6 kJ and AS° =-198.7 J/K at 315 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 315 K. The standard enthalpy change for the reaction of 1.84 moles of N2(g) at this temperature would be kJ.
Measurements show that the energy of a mixture of gaseous reactants decreases by 206. 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 -145. kJ of work is done on the mixture during the reaction. Calculate the change in enthalpy of the gas mixture during the reaction. Be sure your answer has the correct number of significant digits. O exothermic Is the reaction exothermic or endothermic? O endothermic
What is the specific heat capacity of a substance of mass 176.1 g that increases in temperature from 20.8 °C to 27.7 °C after absorbing 2.76 kJ of energy in the form of heat? Express your answer in J g-1 °C-1. Do not try to identify the substance. Express answer in 2 significant figures.
According to Hess's law, what will be the total change in enthalpy for the reaction: Cs. diamond) C(s, graphite) C(s, graphite) + O2(g) → CO2(9) C(s, diamond) + O2(g) AH, = -393.5 kJ AH2 = -395.4 kJ %3D → CO2 (g) %3D O 788.9 kJ O -788.9 kJ O 1.9 kJ O1.9 kJ