Answer:
La reacción de etano, CH₃CH₃ y cloro, Cl₂ en presencia de luz solar se conoce como reacción de halogenación.
Los radicales de cloro se forman cuando el cloro se expone a la luz solar a continuación;
Cl₂ → 2Cl *
Se forma un radical etano cuando el etano, C₂H₆ reacciona con un radical libre de cloro, Cl *, como sigue;
C₂H₆ + Cl → C₂H₅ * + HCl
Se forma un producto halogenado cuando un radical libre de etano reacciona con una molécula de cloro como sigue;
C₂H₅ * + Cl₂ → C₂H₅Cl + Cl *
Un producto halogenado puede reaccionar además con un radical libre para producir como sigue;
C₂H₅Cl + Cl * → C₂H₅Cl₂
Explanation:
Answer:
a) ΔU = 71 kJ
b) the pressure will be higher
Explanation:
Step 1: Data given
A gas does 171 kJ of work on its surroundings
At the same time there is 242 kJ of heat added to the gas
Step 2: Calculate change of internal energy
Change of internal energy ΔU by the gas due to the 171 kJ work done by the system and addition of 242 kJ heat to the system.
heat energy (ΔH) is the summation of heat capacity (ΔU) and work done by a system
ΔU = Q + W
The work is done by the system on its surroundings, what means energy is lost. W will have a negative value: -171 kJ
The heat is added to the system, this means we gain energy. Q will have a positive value: 242 kJ
Total change of intern energy will be:
ΔU = Q - W
ΔU = 242 kJ - 171 kJ
ΔU = 71 kJ
ΔU = nR*ΔT
For an ideal gas n and R are constant. . Now consider PV = nRT.
P and T are directly related. Therefore, an increase in temperature will result in a higher pressure.
Bestie since it’s Cl2, put 2 next to KCl. That means you need to 2 moles of K, so put 2 next to KI. That’s it
Answer:
For 0.5 moles of oxygen consumed, there will be 1.0 moles of H2O produced.
Explanation:
Step 1: Data given
Number of moles of oxygen (O2) = 0.5 moles
Suppose H2 is in excess
Step 2: The balanced equation
O2 + 2H2 → 2H2O
Step 3: Calculate moles of H2O
For 1 mol of O2 we need 2 moles of H2 to produce 2 moles of H2O
For 0.5 moles of O2 we'll have 2*0.5 moles = 1.0 moles of H2O
For 0.5 moles of oxygen consumed, there will be 1.0 moles of H2O produced.
