determine how much heat is released for every 1.00 g of sucrose oxidized from the following: Sucrose C12H22O11 is oxidized in the body by O2 that ultimately produces CO2(g) and H2O (g) and releases 5.64 E3 kJ/mol sucrose. This is what I come up with for the balanced equation: 1 C12H22O11 (s) + 12 O2 (g) ----- 12 CO2 (
The specific heat of fusion of silver is 30.0 calories per gram and the specific heat of silver is 0.30 Joules per gram per degree C. Calculate the energy required to melt 5.0 moles of silver if it starts as a solid at 25 degree C below its normal melting point and is heated to exactly 0.01 Celsius degree above its normal meltin
Thinking about entropy as disordered states, which of the following reactions would show an increase in entropy? Mark those in which entropy increases as TRUE. None of these reactions are balanced. H2 + O2 → H2O 1. True 2. False CaCO3 → CaO + CO2 1. True 2. False H2O(l) → H2O
Which of the following metals would be the least safe to drop in water? Why? A. lithium B. magnesium C. iron D. potassium E. aluminum.
In a particular reaction, the system does work on the surroundings and absorbs heat rom the surroundings. What is the sign of the internal energy change, ^U? A. always negative B. always positive C. positive or negative depending on the relative magnitudes of the energy transfers D. always zero
The correct equation for which the enthalpy change defines the standard enthalpy of formation for C2H5OH (l) is : A. CH2 + CH2 + H2O -->CH3CH2OH B. CH3CHO + H2 -->CH3CH2OH C. 4 C + 6 H2 + O2 --> 2 CH3CH2OH D. 2C + 3H2 + 1/2 O2 -->2 C2H5OH E. 2C + 6H + O --> C2H5OH
For the following reaction, what is the enthalpy of cyclization per mole of actylene? 3C2H2 (g) --> C6H6 (l) ^H = -630 kJ A. 210 kJ/mol C2H2 B. -630 kJ/mol C2H2 C. 0 kJ/mol C2H2 D. -210 kJ/mol C2H2 E. -1890 kJ/mol C2H2
At 25 degrees C and constant pressure, carbon monoxide gas combines with oxygen gas to give carbon dioxide gas with the evolution of 10.1 kJ per gram of carbon monoxide consumed. What is the value of ^H for the balanced reaction? A. -566 kJ/MOL B. -283 kJ/MOL C. 283 kJ.MOL D. 141 kJ/MOL E. -141 kJ/MOL
What mass of oxygen gas, measured at 238 K and 3.51 atm, is required in ordered to release 6670 kJ of heat to the surroundings? CH4 + 2O2 --> CO2 + 2H20 ^H = 890.3 kJ A. 240 B. 6260 C. 0.574 D. 479 E. 7.49
Calculate the heat capacity of a sample of radiator coolant if a temperature rise from -5 degrees C to 142 degrees C requires 932J of heat? A. 0.158 J/C B. 1.37 x 10 to the power of 5 J/C C. 6.80 J/C D. 6.56 J/C E. 6.34 J/C
A 15.) g block of aluminum at an initial temperature of 27 C absorbs 0.678 kJ of heat. What is the final temperature of the block? The specific heat of Al is 0.902 J g-1C-1. A. 50.1 C B. 38.6 C C 54.5 C D. 68.6 C E. 77.6 C.
Copper clips are sometimes used as "heat sinks." How many grams of copper must be in contact with an electric component to absorb 10.0 J of heat and not let the temperature increase by more than 40 C? The specific heat of copper is 0.385 J/g K.
Calcium carbide (CaC2) reacts with water to form acetylene (C2H2), a gas used as a fuel in welding: CaC2 + 2H2O ==> C2H2 + Ca(OH)2 ^H = 128.0 kJ How many kilograms of CaC2 are consumed in a raction that releases 3.64 x 104 kJ of heat under these conditions? A. 1.82 x 10 to the power of 4 kg B. 284 jg C. -18.2 kg D
What is the final temperature of a 52 gram glass of water at 2.0 C, if it absorbs 3.0 J heat? A. -2.0 B. -210 C. 150 D. 2.0 E. 75
The specific heat of aluminum is 0.902 J g-1 C-1 at 25 C. How much heat, in kJ, does it take to raise the temperature of a 12.0 g chunk of aluminum from 15.5 C to 35.5 C? A. 0.216 kJ B. 0.0108 kJ C. 0.0180 kj D. 240 kJ E. 216 kJ
Which of the following liquids has the highest specific heat capacity? water, alcohol, glycerine, or hexane. If you applied equal amounts of heat to equal masses of water and alcohol, which will stay closest to its initial temperature?
A burner on an electric range has a heat capacity of 345 J/K. What is the value of q (heat released) in kilojoules, as the burner cools from temperature of 467 degrees celsius to 23 degrees celsius. A. -153 kJ B. +153 kJ C. -531 kJ D. -431 kJ
WHAT MASS OF WATER CAN BE HEATED FROM 5.5 DEGREES C TO 55.O DEGREES C BY 9.09 x 10^10 J of heat?
When using a calorimeter to do detailed heat calculations, you must determine the heat capacity of the individual calorimeter you use as a calibration factor for later experiments. The fluid in a bomb calorimeter was heated for 568 seconds with a 15.00-watt heater. The temperature of the calorimeter fluid increased by 2.00 deg
A jeweler heats 60 g of gold (about 2 oz) almost to melting, 1000 degrees Celsius and drops it a cold cup of coffee to heat it up. If the cup has 200 ml of liquid in it (treat it as pure water) and is at 25 degrees Celsius before the hot gold is dropped in, estimate the temperature after the gold has been added. The specific hea
The calorie is an energy unit equal to about 4.2 joules. It is defined as the amount of heat required to raise one gram of water by one degree Celsius. An average person has a mass of around 68 kg. About how much energy would be required to raise an equal mass amount of water from room temperature (24 degrees celsius) to body
The decomposition of solid potassium chlorate by heating yields solid potassium chloride and oxygen gas products. Write a balanced equation for this reaction.
1. Before spectroscopy was invented, Korner's absolute method was used to determine whether a disubstituted benzene derivative was the ortho, meta, or para isomer. Korner's method involves adding a third group (often a nitro group) and determining how many isomers are formed. A turn-of-the-century chemist isolated an aromat
General Information: The recrystallized adduct appeared as white, thin, long crystals weighing 0.3606 g and with a melting point of 123-126C. Based on the melting point ranges of the adduct sample, it was concluded that the unknown diene was alpha-phellandrene. DIRECTIONS: 1. DRAW the structure of the alpha-phellandr
Calculate the change in internal energy (DU), heat (q) and work (w) when one kg of Ne is heated from 300 K to 400 K (a) at constant pressure (b) at constant volume (Assume an ideal gas)
If an aluminum sphere has a mass of 23.01 grams and was heated to 137.0 Celsius and lowered into a cup containing 20.00 mL of water at 21.0 Celsius. The final temperature of the water and the sphere was 44.0 Celsius assuming no heat was loss calculate the specific heat of the aluminum in the sphere. C h2o =4.184J/g-0celsius
Write the balanced formulas for the reactants and predicted products for the chemical reactions that follow. Also include net ionic equations. a.) A solution of formic acid, HCOOH, is oxidized by an acidified solution of potassium dichromate. b.) Concentrated hydrochloric acid solution is added to solid manganese(IV) oxide a
1.) Given the following data: Fe2O3(s) + 3CO(g) ---- 2Fe(s) + 3CO2(g) delta H = -23 kJ 3Fe2O3(s) + CO(g) ----- 2Fe3O4(s) + CO2(g) delta H = -39 kJ Fe3O4(s) + CO(g) ----- 3FeO(s) + CO2(g) delta H = +18 kJ Calculate delta H for the reaction FeO(s) + CO(g) ----- Fe(s) +CO2(g) 2.) At 298
1.) Calculate the heat of combustion for the reaction in which ethane combines with oxyen to give carbon dioxide and water vapor. C2H6 + 7/2 O2 ----- 2CO2 + 3H2O a.) 2C(s) + 3H2(g) ----- C2H6(g) delta H = -20.2 Kcal b.) C(s) + O2 (g) ------- CO2(g) delta H = -94.0 Kcal c.) H2(g) + 1/2 O2 ----- H2O(g) delt
1.) The specific heat of a solution is 4.18 J/(grams x degrees Celsius) and its density is 1.02 g/mL. The solution is formed by combining 20.0 mL of solution A with 30.0 mL of solution B, both initially at 21.4 degrees Celsius. The final temperature is 25.3 degrees Celsius. Calculate the heat of reaction. assuming no heat i