Answer:
Pressure = 73.49 atm
Explanation:
The balance chemical equation is as follow,
C₃H₈ + 5 O₂ → 3 CO₂ + 4 H₂O
According to balanced equation,
1 mole of C₃H₈ on combustion gives = 3 moles of CO₂
So,
2 moles of C₃H₈ on combustion will give = X moles of CO₂
Solving for X,
X = 2 moles of C₃H₈ × 3 moles of CO₂ ÷ 1 mole of C₃H₈
X = 6 moles of CO₂
Now, in second step we will calculate the the pressure exerted by CO₂ at 2.5 L volume and 373 K temperature. For this we will use Ideal gas equation assuming the gas is acting as an ideal gas. Therefore,
Data:
Temperature = T = 373 K
Volume = V = 2.5 L
Moles = n = 6 mol ∴ As calculated above.
Gas Constant = R = 0.0821 atm.L.mol⁻¹.K⁻¹
Formula Used:
P V = n R T
Solving for P,
P = n R T / V
Putting Values,
P = 6 mol × 0.0821 atm.L.mol⁻¹.K⁻¹ × 373 K ÷ 2.5 L
P = 73.49 atm
The proper name for PCI6 is phosphorus hexachloride. Therefore it’s true
<span>1. Physical properties
. Its soft
. Its moldable
. Its white/translucent without color added
. Its insoluble in water
. its soluble in benzene and ether
. it melts around 120 degrees farenheit
2. Chemical properties
. It is a hydrocarbon with around 25 carbon atoms
. it reacts with oxygen to form water vapor and CO2
. its nonpolar (not sure if thats physical or chemical)</span><span>
</span>
Answer:
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im 100% sure
Explanation: