Answer :
Answer:
To find the temperature at which the reaction occurred, we can use the ideal gas law equation:
PV = nRT
Given:
Ethene (C2H4) = 61.2g
Oxygen (O2) = 51.7g
Carbon dioxide (CO2) is produced
Water vapor (H2O) is produced
Volume of carbon dioxide = 16 liters
Pressure of carbon dioxide = 724 torr
R = 0.0821 L.atm/(K.mol) (gas constant)
First, determine the moles of CO2 produced using the stoichiometry of the reaction between ethene and oxygen.
Calculate moles of ethene (C2H4): Moles = Mass / Molar mass Moles of C2H4 = 61.2g / molar mass of C2H4
Calculate moles of oxygen (O2): Moles of O2 = 51.7g / molar mass of O2
Determine the limiting reagent (the reactant that produces less product) by comparing the moles of products that can be formed from the moles of reactants.
Use the ideal gas law to find the temperature:
P = 724 torr = 0.954 atm (converted)
V = 16 L
n = calculated moles of CO2
R = 0.0821 L.atm/(K.mol)
T = ? (temperature in Kelvin)
Substitute the values into the ideal gas law equation and solve for the temperature (T).
This calculation will give you the temperature at which the reaction occurred.
44=0.954×16/0.0821×T
cross multiply
0.954×16 = 44(0.0821×T)
=15.264= 158.9456T
divide both sides by 158.9456
=T=15.264/158.9456
T=0.0960kelvin
Explanation:
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