Answer : The rate of consumption of oxygen = 0.245 mol/s
Solution : Given,
Rate at which Hydrogen burns = 0.49 mol/s
The Reaction is,
In this reaction, 2 moles of hydrogen react with the 1 mole of oxygen.
The rate at which oxygen burns is equal to the half of rate at which hydrogen burns.
Rate at which Oxygen burns = 
× 0.49 mol/s
= 0.245 mol/s
The molecular formula gives us the total number of atoms of the compound. To do this we are going to count each of the atoms.
We have:
C = 4
H = 8
O = 2
So, the molecular formula will be C4H8O2
The empirical formula is the simplest way to represent a molecule, we simplify taking the denominators of the molecule to its simplest form, as they are all multiplies of two we can divide everything by this number and thus we obtain the empirical formula.
So, the empirical formula will be C2H4O
Answer:
-431.5 J/g
Explanation:
Mass of solution = Mass of solute + mass of solvent
Solute is KOH while solvent is water.
Mass of KOH = 16.9 g
Mass of water = 90.8 g
Mass of solution = 16.9 + 90.8
= 107.7 g
Change in temperature (Δt) = 34.27 - 18.5
= 16.2 °C
Heat required to raise the temperature of water is released by dissolving KOH.
Therefore,
Heat released by KOH = m × s× Δt
= 107.7 × 4.18 × 16.2
= 7293 J
Heat released by per g KOH = 7293 J/16.9 g
= 431.5 J/g
As heat is released therefore, enthalpy change would be negative.
Enthalpy change of KOH = -431.5 J/g
Answer:
separation of a liquid mixture into fractions differing in boiling point (and hence chemical composition) by means of distillation, typically using a fractionating column.
