13. The burning of 80.3 g of SiH4 at constant pressure gives off 3790 kJ of...
In a constant-pressure calorimetry experiment, a reaction gives off 21.8 kJ of heat. The calorimeter contains 150 g of water, initially at 25.4°C. What is the final temperature of the water? The heat capacity of the calorimeter is negligibly small.
In a constant-pressure calorimetry experiment, a reaction gives off 23.3 kJ of heat. The calorimeter contains 150 g of water, initially at 23.4° C. What is the final temperature of the water? The heat capacity of the calorimeter is negligibly small.
A metal object at 54.0 oC is heated by gaining 30.2 kJ of heat from the environment. The heat capacity, C, of the metal object is 6.30 kJ/ oC When 11.53 g C2H6O (g) is reacted according to the following equation, 368 kJ of heat is released. What is the ΔH of the reaction? C2H6O (g) + 3O2(g) --> 2CO2(g) + 3H2O (l) When 2.45 g of CH3OCH3 is burned at constant Pressure, 77.42 kJ of heat is given off. What is...
Burning propane gives off 49.9 kJ of heat energy per gram. I(f you burn 38.2 g of propane, how much heat energy is released.
1. The standard enthalpy change for the combustion of mole of propane is -2043.0 kJ. CH_(g) +5 0 (g) →3002(g) + 4H2O(g) Calculate Hº for propane based on the following standard molar enthalpies of formation. molecule CO (9) H2O(g) AH (kJ/mol-rxn) -393.5 -241.8 a. +1407.7 kJ/mol-rxn b. +104.7 kJ/mol-rxn c.-104.7 kJ/mol-rxn d -4190.7 kJ/mol-rxn e. -1407.7 kJ/mol-rxn 2. Which of the following statements is/are CORRECT? 1. If a reaction occurs at constant pressure, 4-AH. 2. The change in energy for...
The "roasting" of 48.7 g of ZnS at constant pressure gives off 220. kJ of heat. Calculate the DH for this reaction.2ZnS(s) + 3O2(g) ® 2ZnO(s) + 2SO2(g)A.) -110 kJ/mol rxnB.) -293 kJ/mol rxnC.) -440. kJ/mol rxnD.) -881 kJ/mol rxnE.) +440. kJ/mol rxn
When 20.00 moles of H2(g) reacts with 10.00 mol of O2(g) to form 20.00 mol of H2O(1) at 25°C and a constant pressure of 1.00 atm. If 1366 kJ of heat are released during this reaction, and PAV is equal to -74.00 kJ, then AH° = +1366 kJ and AE = +1440 kJ. O AH° = +1366 kJ and AE° = +1292 kJ. O AH° = -1366 kJ and AE° = -1292 kJ. O AH° = -1366 kJ and AE°...
4. If NaHe ()+ Oz (g) Na (g)+ 2 HO (0) Ha (g) +% O (g) H:O (1) Hz (g)+ O2 (g) H2O: () Find AH for N He ()+2 HzO2 (I) N: (g) +4 H2O () AH 622 2 k/mol AH-285 8 kJ/mol AH-187 8 kJ/mol 5. Using standard heats of formation, calculate AH for 4 FeO (s)+ O2 (g) 2 Fe:Os (s) -272.0 kJ/mol AH'r of FeO (s) AH'r of FeaOs (s) = -825.5 kJ/mol 6. Using standard...
A 0.2075−g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has a heat capacity of 3024 J/°C. The temperature increases by 1.700°C. (a) Calculate the heat given off by the burning Mg in kJ/g. kJ/g (b) Calculate the heat given off by the burning Mg in kJ/mol. kJ/mol
Metal oxides can be reduced with hydrogen gas to give the metal. H2(g) ZnO(s) H2O(g) +Zn(s) Compound Ha(g) Zno AH(kJ/mol) AG (kJ/mol) S (J/Kemol) 130.7 -348.3 43.6 -318.3 H2O(g) Zn(s) -241.8 188.8 -228.6 41.6 What is the entropy change for the reaction? Errent 13 56.1 J/K 2. -56.1 J/K Cacb180.8)- (u 190.) 3. 404.7 J/K 43.6 J/K 4. Metal oxides can be reduced with hydrogen gas to give the metal. H2O(g) +Zn(s) H2(g)+ZnO(s) AG (kJ/mol) AH (kJ/mol) S(J/Kemol) 130.7 Compound...