Phase and State Changes refer to the transformation of a thermodynamic system from one phase or state to another.
In a Reaction Mechanism, a Reaction Intermediate is a molecular entity that is formed by the reactants which reacts further to form the products.
Hess’s Law states that the total enthalpy change accompanying a particular chemical reaction is independent of the pathway between the initial and final states.
Raoult’s Law states that the vapor pressure of an ideal solution is dependent on the vapor pressure and mole fraction of each chemical component in the solution.
The Law of Conservation of Mass states that for any system closed to all transfers of mass and energy, the mass of the system must remain constant over time.
Consider a physical explanation for the difference of vapour pressure of miscible and immiscible solutions. For immiscible the total vapour pressure is equal to the sum of the pressure from the pure liquids but and miscible liquids pressure vapour pressure follows raoults law. What is the physical justification for this?
I have a question about relations for a process even though I am unsure about the scope of this. Still I wonder about a mathematical relation for the following: I wonder about how one defines mathematically that a process is reversible for a process that has both pressure and temperature differences from definition of total e
Question #1 A 25.000g sample of unknown metal is heated to 99.5 degrees Celsius and added to 50.0mL of water in a calorimeter, which has an initial temperature of 22.o degrees Celsius (density of water is 0.99780 g/mL. The temperature of the calorimeter increases to a maximum temperature of 33.5 degrees Celsius. The heat capa
Using the data sheet (see attachment) calculate delta S values for the following reactions. In each case explain the sign of delta S. N2H4(g) + H2(g) --> 2NH3(g) 2Al(s) + 3Cl2(g) --> 2AlCl3(g) Mg[OH]2(s) + 2Hcl(g) --> MgCl2(s) + 2H20(l) 2CH4(g) --> C2H6 + H2(g)
1. For the reaction 2 NO(g) + O2(g) -->2 NO2(g) deltaH = -126.0 kJ at 25C. (a) Calculate the amount of heat transferred when 333 g of NO(g) reacts with O2(g) at 25C and 1 atm. (b) Does this heat flow into the system or does it flow to the surroundings? (c) Is this reaction exothermic or endothermic? 2. If 8675 J of
Two problems that involve calculating the value of a freezing point and to prove a statement about A statistical thermodynamic model of binary solutions.
1. If the vapor pressures of the two components in a binary solution are grven by P1 = x1*P1*e^(u(x2^2))/RT and P2 = x2*P2*e^(u(x1^2))/RT Show that, Del(mix)*G/u = Del(mix)*G/(n1+n2)u = (RT/u) * (x1 ln(x1) * x2ln(x2))*x1x2 Del(mix)*S/R = Del(mix)*S/(n1+n2)R= -(x1 ln(x1) * x2ln(x2)) Del(mix)*H/u = Del(mix)*H/(n1+n2) = x1
The equation of state of one mole of a van der Waals gas is given by (P+a/(v^2))(V-b) = RT with a and b are constants. a) Calculate the work W in an isothermal reversible process when volume changes from V1 to V2. b) Using the energy equation, show that (du/dV) = a/v^2 c) Calculate the change in internal energy U in th
1-HgO(s) Hg(l) + O2(g) Consider the unbalanced equation above. A sample of impure mercury(II) oxide is heated and the HgO decomposed completely. If 680. mL of O2 is collected by displacement of water at a barometric pressure of 680.0 mm Hg and 25.0°C, what mass of HgO was originally present? The vapor pressure of water is 23.
1. Consider the phase change: C(graphite) <---> C(diamond) Given that delta_rG^o/Jmol^-1 = 1895 + 3.363T, calculate the enthalpy and entropy. Calculate the pressure at which diamond and graphite are in equilibrium with each other at 25 degree Celsius. Take the density of diamond and graphite to be 3.51 g/cm^3 and 2.25 g/c
Thermal Interactions Part 1: In an insulated container, you mix 200. g of water at 80ºC with 100. g of water at 20ºC. After mixing, the temperature of the water is 60ºC. a. How much did the temperature of the hot water change? How much did the temperature of the cold water change? Compare the magnitudes (positive values) o
You are out camping with your family and you decide that you would heat some water for cooking your food. The pot you use is made from aluminum (heat capacity, s, = 0.902 J/g@EC). The pot has a mass of 675.6 g and a capacity of 1.356 L. You are going to heat water (s = 4.184 J/g degrees C) starting from ice (s = 36.93 J/mol degr
At 100 degrees Celsius and 1.00 bar, 1.00 mol of liquid water is converted to 1.00 mol of gas. a) Calculate delta Hm, delta Sm and delta Gm. (Look up the standard enthalpy of vaporization at the normal boiling point. Give your source). b) 1.00 mol of liquid water is placed in a previously evacuated chamber at 100 degrees Cel
Please help with the following problem. Many power plants produce energy by burning carbon-based fuels, which also produces carbon dioxide. Carbon dioxide is a greenhouse gas, so over-production can have negative effects on the environment. Use enthalpy of formation data to calculate the number of moles of CO_2 (g) produce
Calorimeter experiment: Refer to attachments for full experimental design. I need help with the following questions: 1. Why is it necessary to start this experiment with a large excess of ice in the metal ice container (the calorimeter)? 2. If all the ice melts when you were doing this experiment so at the end of the
103. Three common hydrocarbons that contain four carbons are listed here, along with their standard enthalpies of formation 1,3 Butadiene, C4H6(g), 111.9 Kj/mol 1-Butene, C4H8 (g), 1.2 Kj/mol n-butene, C4H10(g) -124.7Kj/mol heat formation a) For each o these substances calculate the molar enthalpy of combustion to CO
Calculate the activity coefficient for a liquid mixture that is in equilibrium with its vapors using both Raoult's law and Henry's law
Activity coefficients are used to calculate the actual concentration of non-ideal solutions. When two liquids are mixed together in different mole fractions, the mole fractions of their vapors will also be different. The partial pressures of each component is measured in both the liquid and vapor phase. With a knowledge of both
Please help answer the following question. What mass of water at 100 degrees Celsius would raise the temperature of 30.00g of water at 23.0 degrees C to 32.6 degrees C? For this question, assume that the calorimeter does not absorb any heat. (please show the work)
The complete combustion of acetic acid, HC2H3O2(l) to form H2O(l) and CO2(g) at a constant pressure releases 871.7kJ of heat per mole of HC2H3O2. a) Write a balanced thermochemical equation for this reaction. The answer is HC2H3O2(l) + O2(g)---->2 H2O(l) + 2 CO2 Change (^) H = -871.7kJ b) My question is, if I onl
Please help answer the following thermodynamics questions. a) When a 3.88g sample of solid ammonium nitrate dissolves in 60g of water in a coffee-cup calorimeter, the temperature drops from 23 degrees C to 18.4 degrees C. Calculate ^H (in kJ/mol NH4NO3) for the solution process NH4NO3(s)---->NH4(aq) + + NO3 - Assu
** Please see the attached file for the full problem description **
I am having trouble setting up the follow problems. I am not even sure where to start. If anyone can offer any advice, I would greatly appreciate it, as I am completely stumped: 1) The volume in Liters of H2(g), measured at 22 degrees C and 745 mmHg, required to react with 30.0 L of CO (g), measured at 0 degrees C and 760 mmH
State all of the assumptions (e.g. ideal gas etc). (a) Starting with dGm = VmdP-SmdT, derive the relationship (Clayperon Equation) that expresses the slopes between the solid/liquid/gas phase boundaries in a Pressure versus Temperature plot. (b) Using the Clayperon equation from part a, justify the difference in the solid-li
State all assumptions (e.g. ideal gas etc). Given the followin skeletal reaction for the combustion of hydrogen to generate water using the tables attached to the test: 2H??2(g) + O2(g) ----> 2H2O(g) (a) Determine the Î"HO, Î"So, and Î"Go for the above reaction at 298 Kelvin at 1 bar pressure. (b) Justify and compare
Please help answer the following questions. See the attached file for multiple choice options. 1. Which sample of sulfur at 25°C has the greatest entropy? 2. What is the standard free energy change for the following reaction at 25°C: C(diamond) ---> C(graphite) 3. Which sample of H2O has the least entropy? 4. Which su
Could you please take a look at this? I'm having trouble with #2 and #3. Thank you! Observations: #1 - Initial temperature of Iron shot (Fe) metal: 100°C Final temperature of Iron shot (Fe) metal: 28°C Initial temperature of water from calorimeter: 20°C Final water temperature from calorimeter: 28°C #2
Define chemical potential, equilibrium Constants Kp and Kc. Also derive Kc and Kp mathematically and show the relationship between them.
For the equilibrium system CO2(g) + H2(g) CO(g) + H2O(g) H = +42 kJ/mol K equals 1.6 at 1260 K. If 0.15 mol each of CO2, H2, CO, and H2O (all at 1260 K) were placed in a 1.0-L thermally insulated vessel that was also at 1260 K, then when the system came to equilibrium, A) the temperature would remain constant and the
1.Calculate the amount of heat that must be absorbed by 10.0 g of ice at -20 C to convert it to liquid water at 60.0 C. Given: Specific heat (ice)=2.1 J/goC Specific heat(water)=4.18 J/goC H (fus)=6.0 kJ/mol 420 J 2,900 J 6,300 J 63 kJ 7.5 J 2. The major enthalpy of Boron tribromide (BBr3) is 30.5 kJ/mol, and its norma
Please explain the relationship between calories, food, and heat by responding to the following prompts: 1. List the 'magic formula' for weight loss. List a high-calorie food and a low calorie food. Do you see a relationship between the high calorie foods and the low calorie foods (other than the number of calories?) I ca
a) What is the expression for the eqilibrium constant K in terms of the concentrations of the products and reactants for the reaction between ammonia, (NH3 (aq)) (SMALL 3), WHICH REACTS WITH WATER TO PRODUCE AMMONIUM (NH4 + (aq)) and hydroxide (OH - (aq)) ions. NH3 (aq) + H20 (l) = NH4+ (aq) + OH- (aq) the enthalpy cha