C6H12 + 9 O2 –> 6 CO2 + 6 H2O
1 answer:
5.76 g of are consumed when
is burned to yield 5.3 grams of
.
A mole is defined as 6.02214076 × of some chemical unit, be it atoms, molecules, ions, or others.
Calculating moles of
Number of mole of =
=
= 0.12 mol
As is clear from the reaction stoichiometry, 9 moles of 6 moles of
.
Calculating the number of moles of
= 0.18 mol
Mass of =5.76 g
Hence, 5.76 g of are consumed when
yield 5.3 grams of
.
Learn more about mole here:
#SPJ1
You might be interested in
Answer:
The value of is 0.02495.
Explanation:
Initial concentration of gas = 0.675 M
Initial concentration of gas = 0.973 M
Equilibrium concentration of mustard gas = 0.35 M
initially
0.675 M 0.973 M 0
At equilibrium ;
(0.675-0.35) M (0.973-2 × 0.35) M 0.35 M
The equilibrium constant is given as :
The relation between and
are :
where,
= equilibrium constant at constant pressure = ?
= equilibrium concentration constant =14.45
R = gas constant = 0.0821 L⋅atm/(K⋅mol)
T = temperature = 20.0°C =20.0 +273.15 K=293.15 K
= change in the number of moles of gas = [(1) - (1 + 2)]=-2
Now put all the given values in the above relation, we get:
The value of is 0.02495.
Answer:
6
Explanation:
Formula: Al2O3
If we require 2Al2O3
We divide 2 by 3
Sorry for the shadow of phone and fingers.
