Combustion usually occurs when a hydrocarbon reacts with oxygen to produce carbon dioxide and water. Combustion reactions are almost always exothermic CO(g) + ½O2(g) → CO2(g) + 67.6 kcal
base from the reaction, the stoichiometric ratio is 1 mole CO produce 67.6 kcal so the anwer is - 67.6 kcal because is it exothermic
Answer: strongly acidic
Explanation: a strongly acidic solution has a pH between one and four
If heat flows into the surroundings, the random motions of the molecules in the surroundings increase. Thus, the entropy of the surroundings increases. The second law of thermodynamics states that the total entropy of the universe always increases for a spontaneous process.
Answer:
P2 = 150.4 KPa
Explanation:
Gay-Lussac's Law:
at constant volume, the pressure of a gas varies directly with the temperature
∴ P1 = 55 KPa
∴ T1 = - 100.0°C ≅ 173 K
∴ T2 = 200°C ≅ 473 K
⇒ P2 = ?
⇒ P2 = (473 K)(55 KPa) / (173 K)
⇒ P2 = 150.4 KPa
Answer:
4.75 moles of oxygen would be consumed by water
Explanation:
Given data:
Mass of water produced = 68.1 g
Number of moles of oxygen consumed = ?
Solution:
Chemical equation:
C₃H₈ + 5O₂ → 3CO₂ + 4H₂O
Number of moles of water:
Number of moles = mass/molar mass
Number of moles = 68.1 g/ 18 g/mol
Number of moles = 3.8 mol
Now we will compare the moles of water with oxygen.
H₂O : O₂
4 : 5
3.8 : 5/4×3.8 = 4.75 mol