Balance the equation and then determine the liters of Oxygen need for the complete combustion of...
Balance the equation and then determine the liters of Oxygen need for the complete combustion of 768g of benzene (C6H6) if the reaction is run at 23.5oC and 765mHg? C6H6(l) + O2(g) ⟶ CO2(g) + H2O(g)
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Balance the equation and then determine the liters of Oxygen
need for the complete combustion of...
Balance the equation and then determine the liters of Oxygen need for the complete combustion of...
Balance the equation and then determine the liters of Oxygen need for the complete combustion of 768g of benzene (C6H6) if the reaction is run at 23.5oC and 765mHg? 2 C6H6(l) + 15 O2(g) ⟶ 12 CO2(g) + 6 H2O(g) grams of products (3 sig figs no units):
Show the calculation of the volume of H2O gas formed by the combustion of 18.6 grams...
Show the calculation of the volume of H2O gas formed by the combustion of 18.6 grams of C6H6 at 30oC and 1.10 atm?The combustion of benzene (C6H6) takes place by the following reaction equation. 2 C6H6 (g) + 15 O2 (g) → 12 CO2 (g) + 6 H2O (g) Please Help!
Balance the equation for the complete combustion of ethane: C2H6 (g) + O2 (g) ⟶⟶CO2 (g)...
Balance the equation for the complete combustion of ethane:
C2H6 (g) + O2 (g) ⟶⟶CO2
(g) + H2O (g). Calculate
ΔΔHofor the reaction per mole of
ethane using the given bond dissociation energies.
→CO2(g) + H2O (g). Calculate AH° for Balance the equation for the complete combustion of ethane: C2H6 (g) + O2(g) the reaction per mole of ethane using the given bond dissociation energies. Bond AH” (kJ/mol) C-C 347 H-O 467 C-H 413 O=0 498 C=0 799 CO 358
CH4(g)+O2(g)→CO2(g)+H2O(g) Part A. What coefficients are needed to balance the equation for the complete combustion of...
CH4(g)+O2(g)→CO2(g)+H2O(g) Part A. What coefficients are needed to balance the equation for the complete combustion of methane? Enter the coefficients in the order CH4, O2, CO2, and H2O, respectively. Part B. What mass of carbon dioxide is produced from the complete combustion of 8.30×10−3 g of methane? Part C. What mass of water is produced from the complete combustion of 8.30×10−3 g of methane? Part D. What mass of oxygen is needed for the complete combustion of 8.30×10−3 g of...
1. Balance the equation for the complete combustion of propane gas, which yields carbon dioxide (8)...
1. Balance the equation for the complete combustion of propane gas, which yields carbon dioxide (8) and water (g). (2 points) CzHs (g) + O2(g) → CO2 (g) + H2O (g) Based on your balanced equation above, calculate the volume of oxygen at 45°C and 740 mm Hg that is needed to completely react with 25.0 grams of propane. (7 points)
Hi! I really need help:) a) What is the average molar mass of a mixture of...
Hi! I really need help:)
a) What is the average molar mass of a mixture of gases if
34.6g occupy 45.6L at 57.9 degrees C and 1045 mmHg?
b) Determine the liters of Oxygen needed for the complete
combustion of 769g of benzene (C6H6) if the teaction is run at 23.5
degrees C and 765mHg?
42. What is the average molar mass of a 57.9°C and 1045mmHg? af mass of a mixture of pases if 34.6g occupy 45.0L 43. Determine...
Write a balanced equation for the combustion of benzene, C6H6(l) . If the standard heat of...
Write a balanced equation for the combustion of benzene, C6H6(l) . If the standard heat of combustion of benzene is –3271 kJ/mol. Calculate its standard heat of formation, H°f , given the following data: ( 4 pts) H°f [CO2(g)] = –394 kJ; H°f [H2O(l)] = –286 kJ
C. When exposed to oxygen, fructose undergoes combustion. If you run the reaction with 10.0 g...
C. When exposed to oxygen, fructose undergoes combustion. If you run the reaction with 10.0 g of fructose and 10.0 g of oxygen, how many moles of CO2 can you produce? The unbalanced equation for this reaction is: CeH12O6 + O2 → CO2 + H2O d. You run the reaction in lab and produce 9.49 g of CO,. Did the reaction go to completion? If not, what is your percent yield?
2. Dimethylamine burns in oxygen according to the following equation: 4 C2H7N + 15 O2 →...
2. Dimethylamine burns in oxygen according to the following equation: 4 C2H7N + 15 O2 → 8 CO2 + 14 H2O + 2 N2 (a) How many liters of O2 at 35 °C and 0.840 atm will be needed to burn 7.70 L of C2H7N at 35 °C and 0.840 atm? (b) How many liters of CO2 at 35 °C and 0.840 atm will be produced? Report your answers to parts (a) and (b) to 3 significant figures. 3. Complete...
Balance the equation for the complete combustion of ethane:
C2H6 (g) + O2 (g) ⟶⟶CO2
(g) + H2O (g). Calculate
ΔΔHofor the reaction per mole of
ethane using the given bond dissociation energies.
→CO2(g) + H2O (g). Calculate AH° for Balance the equation for the complete combustion of ethane: C2H6 (g) + O2(g) the reaction per mole of ethane using the given bond dissociation energies. Bond AH” (kJ/mol) C-C 347 H-O 467 C-H 413 O=0 498 C=0 799 CO 358
1. Balance the equation for the complete combustion of propane gas, which yields carbon dioxide (8) and water (g). (2 points) CzHs (g) + O2(g) → CO2 (g) + H2O (g) Based on your balanced equation above, calculate the volume of oxygen at 45°C and 740 mm Hg that is needed to completely react with 25.0 grams of propane. (7 points)
Hi! I really need help:)
a) What is the average molar mass of a mixture of gases if
34.6g occupy 45.6L at 57.9 degrees C and 1045 mmHg?
b) Determine the liters of Oxygen needed for the complete
combustion of 769g of benzene (C6H6) if the teaction is run at 23.5
degrees C and 765mHg?
42. What is the average molar mass of a 57.9°C and 1045mmHg? af mass of a mixture of pases if 34.6g occupy 45.0L 43. Determine...
C. When exposed to oxygen, fructose undergoes combustion. If you run the reaction with 10.0 g of fructose and 10.0 g of oxygen, how many moles of CO2 can you produce? The unbalanced equation for this reaction is: CeH12O6 + O2 → CO2 + H2O d. You run the reaction in lab and produce 9.49 g of CO,. Did the reaction go to completion? If not, what is your percent yield?
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