Find mass of of required when 5.8g
of bulare isburnt ?
CuH10 +o2 -> c02 + H₂0
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Answered by
1
Answer:
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Answered by
0
Answer:
2C
4
H
10
+13O
2
→10H
2
O+8CO
2
Pressure before reaction =P
0
2C
4
H
10
+13O
2
→10H
2
O+8CO
2
At t=0 2 moles 13 moles
At t=t(2−2)(13−13)10moles8moles
= 0 mol = 0 mol of H
2
O(g) of CO
2
At constant volume and temperature :→
PV=nRT
n
P
=
V
RT
constant
n
P
= constant
n
1
P
1
=
n
2
P
2
So, As initial pressure was P
0
P
1
=P
0
initial moles n
1
=15 moles (2+13)
final mole n
2
=18 mole (10+8)
Now,
15
P
0
=
18
P
2
⇒P
2
=
5
6
P
0
Explanation:
hope it helps
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