AssessmentDirections : In a long bond paper, answer the following1. How will you classify photosynthesis, exothermic or endothermic ?justify your answer2. Calculate the AE if 250 kilojoules of heat energy is absorbed by the system and 170 kilojoulesof work is done in the surroundings

In photosynthesis reaction CO2 and H2O reacts to form glucose. 2. q = 250 KJ Work done = - 170 KJ…

Answered: uawssassY Directions : In a long bond…

uawssassY Directions : In a long bond paper, answe 1. How will you classify phot 2. Calculate the AE if 250 kilc of work is done in the surn Ssessme

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 21QRT

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When 2.50 g of methane burns in oxygen, 125 kJ of heat is produced. What is the enthalpy of combustion per mole of methane under these conditions?
When ethanol (grain alcohol, is burned in oxygen, approximately 1360 kJ of heat energy is released per mole of ethanol. mg src=Images/HTML_99425-10-44QAP_image002.jpg alt="" align="top"/> What quantity of heat is released for each gram of ethanol burned? i>What is for the reaction as written? How much heat is released when sufficient ethanol is burned so as to produce 1 mole of water vapor?
9.41 Under what conditions does the enthalpy change equal the heat of a process?
You discover that you cannot carry out a particular reaction for which you would like the enthalpy change. Does this mean that you will be unable to obtain this enthalpy change? Explain.
Ethanol, C2H5OH, is used as a fuel for motor vehicles, particularly in Brazil. (a) Write the balanced equation for the combustion of ethanol to CO2(g) and H2O(g), and, using the data in Appendix G, calculate the enthalpy of combustion of 1 mole of ethanol. (b) The density of ethanol is 0.7893 g/mL. Calculate the enthalpy of combustion of exactly 1 L of ethanol. (c) Assuming that an automobile’s mileage is directly proportional to the heat of combustion of the fuel, calculate how much farther an automobile could be expected to travel on 1 L of gasoline than on 1 L of ethanol. Assume that gasoline has the heat of combustion and the density of n—octane, C8H18(Hf=208.4kJ/mol;density=0.7025g/mL).
9.84 Some claim it would be more logical to use heats of atomization, the energy required to convert any molecule to its separated atoms, rather than heats of formation for doing calculations with Hess's law. If you had a table of heats of atomization and calculated the combustion energy of a fuel, would you get the same answer as you would get using heats of formation? Explain your answer.
What quantity of heat energy must have en applied to a block of aluminum weighing 42.7 g if the temperature of the block of aluminum increased by 15.2 °C? (See Table 10.1.)
The enthalpy change for the reaction CH4(g)+2O2(g)CO2(g)+2H2O(l) is 891 kJ for the reaction as written. a. What quantity of heat is released for each mole of water formed? b. What quantity of heat is released for each mole of oxygen reacted?
Hydrogen sulfide gas is a poisonous gas with the odor of rotten eggs. It occurs in natural gas and is produced during the decay of organic matter, which contains sulfur. The gas burns in oxygen as follows: 2H2S(g)+3O2(g)2H2O(l)+2SO2(g) Calculate the standard enthalpy change for this reaction using standard enthalpies of formation.
In the process of isolating iron from its ores, carbon monoxide reacts with iron(III) oxide, as described by the following equation: Fe2O3(s)+3CO(g)2Fe(s)+3CO2(g)H=24.8kJ The enthalpy change for the combustion of carbon monoxide is 2CO(g)+O2(g)2CO2(g)H=566kJ Use this information to calculate the enthalpy change for the equation 4Fe(s)+3O2(g)2Fe2O3(s)H=?
A 0.470-g sample of magnesium reacts with 200 g dilute HCl in a coffee-cup calorimeter to form MgCl2(aq) and H2(g). The temperature increases by 10.9 C as the magnesium reacts. Assume that the mixture has the same specific heat as water and a mass of 200 g. (a) Calculate the enthalpy change for the reaction. Is the process exothermic or endothermic? (b) Write the chemical equation and evaluate H.
Compounds with carboncarbon double bonds, such as ethylene, C2H4, add hydrogen in a reaction called hydrogenation. C2H4(g)+H2(g)C2H6(g) Calculate the enthalpy change for this reaction, using the following combustion data: C2H4(g)+3O2(g)2CO2(g)+2H2O(l);H=1411kJC2H6(g)+72O2(g)2CO2(g)+3H2O(l);H=1560kJH2(g)+12O2(g)H2O(l);H=286kJ

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