The answer that your looking for is b
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Reaction of combustion of butane is a as follows:
2 C₄H₁₀ + 13 O₂ --> 8 CO₂ + 10 H₂O:
As it can be seen from the equation that 2 mole of butane produce= 8 mole of butane produce
1 mole of butane produce= 4 mole of butane produce
1.60 g of butane=
= 0.027 mole of butane
0.027 mole of butane =
= 0.108 mole of CO₂.
Using ideal gas equation,
Here,
P denotes pressure
V denotes volume
n denotes number of moles of gas
R denotes gas constant
T denotes temperature
The values at STP will be:
P=1 atm
T=23+273 K = 296 K
R=0.0821 atm L mol ⁻¹
Number of moles of gas, n= 0.018
Putting all the values in the above equation,
V= 2.62 L
So the volume will be 2.62 L
Answer:
The new volume is 7,606.96 Liter.
Explanation:
The combined gas equation is,
where,
= initial pressure of gas in the balloon = 0.918 atm
= final pressure of gas in the balloon = 0.0012 atm
= initial volume of gas in the balloon =
= final volume of gas in the balloon = ?
= initial temperature of gas in the balloon =
= final temperature of gas in the balloon =
Now put all the given values in the above equation, we get:
The new volume is 7,606.96 Liter.