Answer:
x = 4.5
4.5 moles of C2H6 is required to produce 13.5 moles of H2O
Explanation:
Given equation is :
2 C2H6 + 7 O2 → 4 CO2 + 6 H2O
if it requires 2 moles of C2H6 to produce 6 moles of H2O
then x moles of C2H6 is required to produce 13.5 moles of H2O
Using unitary method for solving, we get
x = 13.5 x 2 / 6
x = 13.5 / 3
x = 4.5
Therefore, 4.5 moles of C2H6 is required to produce 13.5 moles of H2O
Answer:
Balanced Eqn
2
C
2
H
6
+
7
O
2
=
4
C
O
2
+
6
H
2
O
By the Balanced eqn
60g ethane requires 7x32= 224g oxygen
here ethane is in excess.oxygen will be fully consumed
hence
300g oxygen will consume
60
⋅
300
224
=
80.36
g
ethane
leaving (270-80.36)= 189.64 g ethane.
By the Balanced eqn
60g ethane produces 4x44 g CO2
hence amount of CO2 produced =
4
⋅
44
⋅
80.36
60
=
235.72
g
and its no. of moles will be
235.72
44
=5.36 where 44 is the molar mass of Carbon dioxideBalanced Eqn
2
C
2
H
6
+
7
O
2
=
4
C
O
2
+
6
H
2
O
By the Balanced eqn
60g ethane requires 7x32= 224g oxygen
here ethane is in excess.oxygen will be fully consumed
hence
300g oxygen will consume
60
⋅
300
224
=
80.36
g
ethane
leaving (270-80.36)= 189.64 g ethane.
By the Balanced eqn
60g ethane produces 4x44 g CO2
hence amount of CO2 produced =
4
⋅
44
⋅
80.36
60
=
235.72
g
and its no. of moles will be
235.72
44
=5.36 where 44 is the molar mass of Carbon dioxide
Explanation:
