Explanation:
b is correct. 30.6 g H2O is produced.
26. B
27. D
28. C
Hope this helped ☺️
*Answer:
Option A: 59.6
Explanation:
Step 1: Data given
Mass of aluminium = 4.00 kg
The applied emf = 5.00 V
watts = volts * amperes
Step 2: Calculate amperes
equivalent mass of aluminum = 27 / 3 = 9
mass of deposit = (equivalent mass x amperes x seconds) / 96500
4000 grams = (9* amperes * seconds) / 96500
amperes * seconds = 42888888.9
1 hour = 3600 seconds
amperes * hours = 42888888.9 / 3600 = 11913.6
amperes = 11913.6 / hours
Step 3: Calculate kilowatts
watts = 5 * 11913.6 / hours
watts = 59568 (per hour)
kilowatts = 59.6 (per hour)
The number of kilowatt-hours of electricity required to produce 4.00kg of aluminum from electrolysis of compounds from bauxite is 59.6 kWh when the applied emf is 5.00V
6 CO₂ + 6 H₂O (chlorophyll + sunlight) ⇒ C₆H₁₂O₆ + 6 O₂
the reaction takes place in presence of sunlight and chlorophyll ..
CO₂ is oxidized and forms Glucose . And oxygen is evolved in this process.
