When 20.00 moles of H2(g) reacts with 10.00 mol of O2(g) to form 20.00 mol of...
When 20.00 moles of H2(g) reacts with 10.00 mol of O2(g) to form 20.00 mol of H2O(l) at 25°C and a constant pressure of 1.00 atm. If 1366 kJ of heat are released during this reaction, and PΔV is equal to -74.00 kJ, then
ΔH° = -1366 kJ and ΔE° = -1292 kJ.ΔH° = +1366 kJ and ΔE° = +1440 kJ.ΔH° = -1366 kJ and ΔE° = -1440 kJ.ΔH° = +1366 kJ and ΔE° = +1292 kJ.
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When 20.00 moles of H2(g) reacts with 10.00 mol of O2(g) to form
20.00 mol of...
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...
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°...
How much heat is absorbed/released when 20.00 g of NH3(g) reacts in the presence of excess O2 (g) to produce NO (g) and...
How much heat is absorbed/released when 20.00 g of NH3(g) reacts in the presence of excess O2 (g) to produce NO (g) and H2O (l) according to the following chemical equation? 4NH3 (g) + 5O2 (g) ---> 4NO (g) +6H2O (l) Δ H: +1168 kJ a. 342.9 kJ of heat are absorbed. b. 342.9 kJ of heat are released. c. 1372 kJ of heat are absorbed. d. 1372 kJ of heat are released. Please explain your answer.
When H2(g) reacts with O2(g) according to the following reaction, 242 kJ of energy are evolved...
When H2(g) reacts with O2(g) according to the following reaction, 242 kJ of energy are evolved for each mole of H2(g) that reacts. Complete the following thermochemical equation. 2H2(g) + O2(g)— 2H2O(g) AH- The following information is given for bismuth at latm: T = 1627.00°C T. = 271.00°C Specific heat solid = 0.1260 J/g °C Specific heat liquid = 0.1510 J/g °C AHvap (1627.00°C) = 822.9 J/g AH (271.00°C) = 52.60 Jig A 38.40 g sample of liquid bismuth at...
When 56.8 g of lead reacts with 3.50 L of oxygen gas, measured at 1.00 atm...
When 56.8 g of lead reacts with 3.50 L of oxygen gas, measured
at 1.00 atm and 25.0 0 degrees * C , 60.1 kl of heat is released at
constant pressure. What is AH for this reaction? (R = 0.0821L * atm
/ (Kmol)) 2Pb(s)+O 2 (g) 2PbO(s) )
When 56.8 g of lead reacts with 3.50 L of oxygen gas, measured at 1.00 atm and 25.0°C. 60.1 kJ of heat is released at constant pressure. What is AH°...
A mixture of 2.0 mol of H2(g) and 1.0 mol of O2(g) is placed in a...
A mixture of 2.0 mol of H2(g) and 1.0 mol of O2(g) is placed in a sealed evacuated container made of a perfect insulating material at 24 ∘C. The mixture is ignited with a spark and it reacts to form liquid water. (The specific heat for water vapor is 2.04 J/g⋅oC, and ∆Hvap = 44.0 kJ/mol) The heat generates in the exothermic reaction will heat the liquid water to boiling, vaporize it, and heat the vapor to its final temperature....
DH=DUIDIN 1. In following reaction H2(g) + Cl2(g) + 2HCl(g) AH=- 184.6 kJ/mol If 4 moles...
DH=DUIDIN 1. In following reaction H2(g) + Cl2(g) + 2HCl(g) AH=- 184.6 kJ/mol If 4 moles of H2 react with 4 moles of Cl, to form HCI. Calculate AU for this reaction, assumimg the reaction goes to completion against a pressure of 138.0 atm at constant volume. (IL atm = 101.3 J) pranai DU=q tw A) -738.4 kJ B) -369.2 kJ C) 138.0 kJ D) 184.6 kJ E) 244.5 kJ 4H =-92.3 ou-bH
2CH3OH(g)→2CH4(g)+O2(g),ΔH=+252.8 kJ 1. Calculate the amount of heat transferred when 25.0 gg of CH3OH(g)CH3OH(g) is decomposed...
2CH3OH(g)→2CH4(g)+O2(g),ΔH=+252.8 kJ 1. Calculate the amount of heat transferred when 25.0 gg of CH3OH(g)CH3OH(g) is decomposed by this reaction at constant pressure 2. For a given sample of CH3OHCH3OH, the enthalpy change during the reaction is 82.3 kJkJ . What mass of methane gas is produced? 3. How many kilojoules of heat are released when 38.6 gg of CH4(g)CH4(g) reacts completely with O2(g)O2(g) to form CH3OH(g)CH3OH(g) at constant pressure?
When .514 g of C12H10 undergoes combustion in a bomb calorimeter, the temperature increases from 25.8oC...
When .514 g of C12H10 undergoes combustion in a bomb calorimeter, the temperature increases from 25.8oC to 29.4oC. The heat capacity of the bomb and all of its contents is 5.86 kJ/oC. What is the heat released per mole of C12H10? Is the number you calculated ΔE or ΔH? Why? Is ΔE = ΔH for this reaction? Why? Balanced reaction: 2 C12H10 (s) + 29 O2 (g) → 24 CO2 (g) + 10 H2O (g) If ΔE and ΔH are...
When excess Cl2 at constant pressure reacts with 0.300 mol of CH4(g) 295 kJ of energy...
When excess Cl2 at constant pressure reacts with 0.300 mol of CH4(g) 295 kJ of energy evolves. Calculate the value of ΔH for this reaction, as written. CH4(g) + Cl2(g) → CHCl3(l) + H2(g) ΔH = ? a) -1970 kJ b) -1770 kJ c) +1970 kJ d) -983 kJ e) +1770 kJ
The reaction between hydrogen and oxygen to yield water vapor has ΔH∘=−484kJ: 2H2(g)+O2(g)→2H2O(g)ΔH∘=−484kJ A) How much PV work is done in kilojoules for the reaction of 0.36 mol of H2 with 0.18 mol...
The reaction between hydrogen and oxygen to yield water vapor has ΔH∘=−484kJ: 2H2(g)+O2(g)→2H2O(g)ΔH∘=−484kJ A) How much PV work is done in kilojoules for the reaction of 0.36 mol of H2 with 0.18 mol of O2 at atmospheric pressure if the volume change is -3.8 L ? B) What is the value of ΔE in kilojoules.
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°...
When H2(g) reacts with O2(g) according to the following reaction, 242 kJ of energy are evolved for each mole of H2(g) that reacts. Complete the following thermochemical equation. 2H2(g) + O2(g)— 2H2O(g) AH- The following information is given for bismuth at latm: T = 1627.00°C T. = 271.00°C Specific heat solid = 0.1260 J/g °C Specific heat liquid = 0.1510 J/g °C AHvap (1627.00°C) = 822.9 J/g AH (271.00°C) = 52.60 Jig A 38.40 g sample of liquid bismuth at...
When 56.8 g of lead reacts with 3.50 L of oxygen gas, measured
at 1.00 atm and 25.0 0 degrees * C , 60.1 kl of heat is released at
constant pressure. What is AH for this reaction? (R = 0.0821L * atm
/ (Kmol)) 2Pb(s)+O 2 (g) 2PbO(s) )
When 56.8 g of lead reacts with 3.50 L of oxygen gas, measured at 1.00 atm and 25.0°C. 60.1 kJ of heat is released at constant pressure. What is AH°...
DH=DUIDIN 1. In following reaction H2(g) + Cl2(g) + 2HCl(g) AH=- 184.6 kJ/mol If 4 moles of H2 react with 4 moles of Cl, to form HCI. Calculate AU for this reaction, assumimg the reaction goes to completion against a pressure of 138.0 atm at constant volume. (IL atm = 101.3 J) pranai DU=q tw A) -738.4 kJ B) -369.2 kJ C) 138.0 kJ D) 184.6 kJ E) 244.5 kJ 4H =-92.3 ou-bH
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