A styrofoam calorimeter contains 60.0 mL of 0.750 M H3C6H5O7 at 22.8oC. When 9.83 g NaHCO3 is added to the calorimeter, the temperature of the resulting solution decreases to a minimum of 5.1oC. The reaction that occurs is: H3C6H5O7(aq)+3NaHCO3(aq)→Na3C6H5O7(aq)+3CO2(g)+3H2O(l) ΔHreaction=??? What is the (experimental) enthalpy change for this reaction, ΔHreaction? (Use the total mass of solution and 4.18 J/(g oC) for the specific heat of the solution in your calculations.)

Phosphoryl chloride, POCI3(g), is used in the manufacturing of flame retardants. It is manufactured in an equilibrium process in which phosphorus trichloride reacts with nitrogen dioxide to form POCI3(g)and NO(g) according to the following equation: PCI3 (g) + NO₂ (g) = POCI3 (g) + NO (g) + 228.93kJ At 298K, the equilibrium concentration of POCI3 was 0.68 mol/L, the concentration of NO was 0.72mol/L, the concentration of PCI3 was 0.62 mol/L, and the concentration of NO₂ was 0.56 mol/L. E' - C E a. 6.25 moles of POCI3 (g) is added to the 5.0 L reaction chamber. What is the new concentration of POCI3 (g) when equilibrium is re-established? PCI 3 (g) + NO₂(g) POCI 3 (g) + NO(g) b. What would happen to the Keq value if the temperature of the reaction chamber was decreased from 500K to 298K? Explain. *Note this question is based on the above chemical equation*

Calculate the change in internal energy (in kcal) for the reaction Cl2(g) + 7/2 O2(g) = Cl₂O7(g) at 25 °C, given that the gases are ideal. The enthalpy, AH, for the formation of Cl₂O7(g) is 63.4 kcal mol- ¹ at 25 °C.

When ammonium chloride (NH_(4)Cl) is added to water, it breaks into positive and negative ions and decreases the temperature of the medium. Which statement is TRUE about this reaction?

Please don't provide handwritten solution .....

When 50.0 mL of 1.24 M of HCI(aq) is combined with 50.0 mL of 1.32 M of NaOH(aq) in a coffee-cup calorimeter, the temperature of the solution increases by 8.0 °C. What is the change in enthalpy for this balanced reaction? HCl(aq) + NaOH(aq) → NacI(aq) + H2 O(); Assume that the solution density is 1.00 g/mL and the specific heat capacity of the solution is 4.18 J/g?°C) a. -52.7 kJ O b. -55.3 kJ O C. -56.7 kJ O d. -53.9 kJ O e. -57.8 kJ

Carbon monoxide and nitrogen monoxide gases combine to form carbon dioxide and nitrogen gases according to the following balanced chemical equation: AG rxn 2 CO (g) + 2NO(g) + 2 CO₂ (g) + N₂ (8) = -689.6 kJ What will be the Gibbs free energy change (AGxn) in kJ if the reaction occurs at 39.96 °C? (4 sf) The partial pressures of the gases are: CO: 0.02250 atm NO: 0.01700 atm CO₂: 2.825 atm N₂: 2.915 atm

Provide the formal definition of enthalpy and explain all symbols used in it. Explain how the change in enthalpy is related to certain thermodynamic property (other than Gibbs energy).

When nitroglycerin explodes, the chemical reaction that occurs can be assumed to be C3H5N3O9(1) → 3CO2(g) + 3/2N2(g) + 1/4O2(g). Calculate the work done on the atmosphere (1 atm) by the explosion of 0.25 mol of nitroglycerin at 25°C. Assume that the gaseous products behave ideally.

7. (a A 5.00 mol sample of an ideal gas is compressed irreversibly and isothermally at 150.00 K from an initial volume of 30.00 L in two steps: Step #1: Pext = 5.00 bar, Step #2: Pext = 20.00 bar. Determine the value of the total work and heat involved (in J). (b) Describe in words what happens to the total amount of work if the compression occurs in three steps. (c). Assuming the process could be done in one or multiple steps and the process could be reversible or irreversible, determine the minimum and maximum amount of work that could be done to complete the compression.