From the data listed, calculate the total heat, in Joules, to convert 10.0 g of liquid ethanol at 55.0 C to gaseous ethanol at 95.5 C.
Using Faraday's Law to solve an electrochemical thermodynamics problem, considering an iron sample protected by nickelization
An iron sample (surface area of 3.3 cm^2) was protected by nickelization in a solution containing 0.1 M NiSO4 and 1 M H2SO4 at a current of 0.28 A for 30 min. What will be the sample weight increase after the process of nickelization upon 62% current efficiency? Please show step by step solution.
What is the change in entropy of 1.00 kg of liquid water at 100 degrees C as it changes to steam at 100 degrees C?
5. In the decomposition reaction of gallium chlorate, 450 grams is heated, to produce oxygen and gallium chloride. Calculate the following: 1. Write the balanced equation for the reaction 2. Find the mole ratios of the reactants and products required to solve any stoichiometric problem 3. Find the mass in megagrams of ga
Alumminum metal melts at 660 degree Celsius and boils at 2450 degree C. Its density is 2.70 grams/cc. Calculate the following: the volume occupied by 15 milligrams of aluminum vapor at its boiling point and under a pressure of 1140 torr. the volume occupied by 100 kilograms of the metal at 25 C. If the specific heat ca
1. At 25 degees C, (triange)H(little o) for the combustion of liquid octane, C8H18(l) to form CO2(g) and H2O(l) is -5471kJ/mol. Calculate (triangle)E(little o) for this reaction at 25 degrees C. 2. The molar heat of vaporization of benzene, C6H6, at 1 atm is 30.8 kJ/mol. The boiling point of benzene at 1 atm is 78.3 degree C.
1.) In the reaction CaO(s) + SO2(g) YEILDS CaSO3(s), Which is correct: O2- acts as a Lewis base, and SO2 acts as a Lewis acid. Ca2+ acts as a Lewis base, and SO42- acts as a Lewis acid. SO42- acts as a Lewis base, and SO2 acts as a Lewis acid. SO2 acts as a Lewis base, and O2- acts as a Lewis acid. SO2 act
1. Predict the sign of delta S for the following reaction. Please explain the reason for your prediction. HgS(s) + O2(g) yields Hg(l) + SO2(g)
Heat of combustion of ethanol, calculation of heat of combustion of ethanol.
Carry out a FIVE-STEP SYNTHESIS using a reaction from AT LEAST FOUR BOXES, and any other reaction that you know of anything at all, starting from one molecule having SEVEN carbons and one chiral center, and adding anything with FIVE or fewer carbons in each step (YOU WILL MOST LIKELY ADD NO CARBONS IN AT LEAST ONE OF THE STEPS).
Use the thermochemical equations shown below to determine the enthalpy for the reaction: 2Fe3O4(s) + 1/2O2(g)=>3Fe2O3(s) 6Fe(s) + 9/2O2(g)=>3Fe2O3(s) H=-1387.4KJ 6Fe(s) + 4O2(g)=>2Fe3O4(s) H=-1256.6KJ
Use the thermochemical equations shown below to determine the enthalpy for the reaction: Fe3O4 + CO(g)=>3FeO(s) + CO2(g) 2Fe(s) + 3CO2(g)=>Fe2O3(s) + 3CO(g) H=5.7KJ 2Fe3O4(s) + CO2(g)=>3Fe2O3(s) + CO(g) H=9.7KJ FeO(s) + CO(g)=>Fe(s) + CO2(g) H=0.3KJ
Calculate the enthalpy change of the reaction CH4 (g) + 2Cl2(g) ￼ CCl4 (l) + 2H2 (g), using thermochemical equations: a) C(s) + 2Cl2 (g) ￼ CCl4 (l) ￼ = -128 kJ b) CH4 (g) ￼ C(s) + 2H2 (g) ￼ = + 75 kJ
Calculate the enthalpy change of a reaction using the following values, enthalpy of reactant 1 = 404 kJ, enthalpy of reactant 2 = 432 kJ, enthalpy of product 1 = 218 kJ, enthalpy of product 2 = 74 kJ and enthalpy of product 3 = 199 kJ.
Calculate the enthalpy change for the reaction, NaCl + water ￼ NaOH + HCl. Using the given values, the sum of the enthalpies of NaCl and water = 293 kJ and the sum of the enthalpies of NaOH and HCl = 162 kJ.
Calculate the standard enthalpy change of a reaction using the total enthalpies of the reactants and the products. The total enthalpy of the reactants is -912 kJ and the total enthalpy of the products is -82 kJ.
Calculate the enthalpy change of the reaction 2CO(g) + 2NO(g) ￼ 2CO￼(g) +N￼(g) using thermochemical equations: a) 2CO(g) + O￼(g) ￼ 2CO￼(g) b) 2NO(g) ￼ N￼(g) + O￼(g) The enthalpy of the equation a) is -566.0 kJ and the enthalpy of the equation b) is -180.6 kJ.
When a 50.0-g nugget of pure gold is heated from 35.0°C to 50.0°C, it absorbed 5200.0 J of energy. Find the specific heat of gold.
Step by Step explanation Ferrous oxalate, FeC2O4, will decompose on heating: FeC2O4 (s) ® FeO (s) + CO2 (g) + CO (g) A 1.25-gram sample of FeC2O4 is added to an evacuated 2.00-liter steel vessel. The vessel is heated to 400°C, at which point all the FeC2O4 is decomposed. Calculate the pressure inside the vessel at 400
The gaseous hydrocarbon acetylene, C2H2 is used in welders' torches because of the large amount of heat released when acetylene burns with oxygen, producing carbon dioxide and water.
1. The gaseous hydrocarbon acetylene, C2H2 is used in welders' torches because of the large amount of heat released when acetylene burns with oxygen, producing carbon dioxide and water. First, write a balanced equation fro the combustion of acetylene is oxygen. Then, how many grams of oxygen are needed for the complete combusti
Given the Ka for HCLO is 3.0*10^-8, calculate delta G standard, at 25 degrees C, for : H30+(aq) + ClO-(aq) --> HCLO(aq) + H2O(l)
For a certain complexation reaction, K=10^17. What are the signs of delta H standard, delta S standard and delta G standard for the equation from which the K expression is derived?
1. Which molecule below should have the highest gas-phase absolute entropy at 25°C? a. CH4 b. H2 c. C2H6 d. C2H4 e. C2H2 2. Some standard entropies (at 25°C in J/mol K) are given: Ca2+(aq) -55.2, F-(aq) -9.6, CaF2(s) +68.87. ΔS° for the reaction CaF2(s)  Ca2+(aq) + 2F-(aq) at 25°C in J/K is ____
7.5. Given the following table of thermodynamic data, substance ΔHf° S° POCl3 (g) -542.2 kJ/mol 325 J/mol - K POCl3 (l) -597.0 222 determine the normal boiling point (in °C) of POCl3. a. 133.0 b. 532 c. 273
1. Which one of the following is a correct statement of the first law of thermodynamics? a. ΔS = q - T b.at absolute zero, for a pure crystalline solid, S = O c. ΔS >or equal q/T d. ΔH = ΣΔHproducts - ΣHreactants e. ΔE = q + w 2. A reversible process is one that ________. a. must be carried out at high
When lithium iodide is dissolved in water, the solution becomes hot. If an aqueous solution of LiI together with additional solid LiI were heated, would some of the solid dissolve or would more solid precipitate? I am very confused as to what this means and I can't find anything that really explains it in my book.
You mix together the following solutions in a coffee-cup calorimeter: - 100.0 mL of 0.200 M CsOH - 50.0 mL of 0.400 M HCl Both solutions start out at 22.50°C, and the final temperature after reaction is 24.28°C. The densities of the solutions are all 1.00 g/mL, and the specific heat of the mixture is 4.2 J/g°C. Calculat
You are given 10.0 grams of a mixture of NaNO3 and KF. You dissolve this mixture in 100.0 grams of water, and the temperature rises by 1.02°C. Calculate the mass of each salt in the original mixture. Assume that the specific heat of the solution is 4.18 J/g°C. Useful information: Enthalpy of solution of NaNO3: +20.5 kJ/mol
I need some help with this problem, see attached file for full problem description with proper symbols: 2. a) Use only the following data to determine delta H°f for NO2 (g): - delta H°f for NO (g) is +90.4 kJ/mol - delta H = -56.6 kJ/mol for the reaction: NO (g) + 1/2 O2 (g) ---> NO2 (g) b) Find delta H for the reaction: 4
1. I need help with the standard deviation/percentage error in the attached lab experiment. 2. Also need help graphing for the ethyl acelate and unknown solvent -- plotting negative delta T versus the total volume of solute that was added (2 graphs) and calculation of the slopes 3. I am not certain but I believe this ques