### The heat of evaporation of water is 540 cal/g

The heat of evaporation of water is 540 cal/g. the specific heat is 0.48 cal/g-c. What will final temperature be if 1020 calories are added to 10 g of water originally 100 degree C?

The heat of evaporation of water is 540 cal/g. the specific heat is 0.48 cal/g-c. What will final temperature be if 1020 calories are added to 10 g of water originally 100 degree C?

1. Use Hess's law and the thermochemical equations given below to calculate the standard enthalpy change for the reaction between C2H4 and F2. (see attached for formatted remainder) 2. (Hess's Law) Thermochemical tables tell us that the conversion of one mole of diamond to one mole of graphite is accompanied by the re

Ethanol, C2H5OH, melts at -114 degrees C and boils at 78 degreesC. The enthalpy of fusion of ethanol is 5.02kj/mol and the enthalpy of vaporization is 38.56kj/mol. The specific heats of solid and liquid ethanol are 0.97J/g-K and 2.3J/g-K respectively. How much heat is required to convert 75.0g of ethanol at -120 degreesC to t

A bowl of oil and a bowl of water have been placed under a heat lamp. The temperature of each was recorded every 5 minutes in the chart below. Using the data from the chart can you determine which absorbed more heat energy? Which has the highest specific heat? If you were to plot the data on a graph using 2 lines (one fo

If ΔG is negative, a reaction is spontaneous in the forward direction. A reaction that is not spontaneous at low temperature can become spontaneous at high temperature if ΔH is ________ and ΔS is ________. a. -, - b. +, + c. +, 0 d. -, + e. +, - Which one of the following statements is true about the equilibrium

Calculate the maximum concentration (in M) of sulfide ions in a solution containing 0.181 M of lead ions. The Ksp for lead sulfide is 3.4 x 10-28. a. 1.9 x 10-27 b. 9.4 x 10-28 c. 1.5 x 10-26 d. 3.0 x 10-25 e. 3.4 x 10-28 A reaction that is spontaneous ___________. a. will proceed as written without outside interv

What are the ΔHf (kJ/mol) and ΔS (J/K*mol) values for Cr3+(aq).

1. How much N2 can dissolve in water at 25'C if the N2 partial pressure is 585. Mm Hg? 2. Hexachlorophene is used in germicidal soalp. What is its molar mass if 0.640g of the compound, dissolved in 25.0 g of chloroform, produces a solution whose boiling point is 61.93 'C? 3. The enthalpy of solution of KClo3 in water is

3.) Show the reaction coordinate diagram (energy diagram) for the process in which the energy change of the reaction is -60 kJ, and the activation energy is 30 kJ. What is the reverse process activation energy?

Using the heat of combustion of octane C8H18 (l) -5470.5 and heat of formation table determine the enthalpy formation value for octane.

What is the final temperature of a calorimeter in which 5.6g of copper at 354 K is put into 56.8 g of water at 22.4 degrees centigrade?

1) Describe in detail the difference in absolute entropy values for the following pairs: a) C(s, graphite) and C(s, diamond) b) HCl(g) and HCl(aq) c) CH4(g) and CH3CH2CH2CH3(g) 2) a) Calculate the values of DeltaH° and DeltaS° for the following reaction at 25°C. b) Use the values from a to calculate DeltaG° for the

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.

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.

You have been handed an unknown, pure chemical substance. Explain how you would identify it.

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

Calculate delta S for the reaction: 4 Cr(s) + 3 O2(g) yields 2 Cr2O3(s) Substance Cr(s) O2(g) Cr2O3(s) S (J/K mol) 23.77 205.138 81.2

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.

Hydrogen peroxide decomposes according to the following thermochemical reaction: H2O2(l) --> H2O(l) + 1/2 O2(g); DH = -98.2 kJ Calculate the change in enthalpy, DH, when 1.00 g of hydrogen peroxide decomposes.

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).

The vapor pressure of a liquid in the temperature range 200 to 260K was found to fit the expression ln( P/torr) = 16.255 - (2501.8 / T/K) Calculate the enthalpy of vaporization of the liquid.

When some large nuclear plants run at full capacity, they produce about 1900 MW of electrical power. At this rate, what mass of 235U (kg) would it consume per year if the efficiency of converting nuclear energy to electricity is 33%? How many metric tons of coal would be required to supply the same amount of electricity?

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