A sample of C2H4 with a pressure of 1.78 atm and a volume of 295 mL is allowed to react with excess H2 at 151 °C. H2 (g) + C2H4 (g) C2H6 (g)
Calculate the pressure of the C2H6 produced in the reaction if it is transferred to a 2.62-L flask and cooled to 34 °C.
Step 1: calculate number of mol of C2H4
Given:
P = 1.78 atm
V = 295.0 mL
= (295.0/1000) L
= 0.295 L
T = 151.0 oC
= (151.0+273) K
= 424 K
find number of moles using:
P * V = n*R*T
1.78 atm * 0.295 L = n * 0.08206 atm.L/mol.K * 424 K
n = 1.509*10^-2 mol
Step 2: Calculate number of mol C2H6
The balanced reaction is:
H2 (g) + C2H4 (g) —> C2H6 (g)
So,
mol of C2H6 produced = mol of C2H4
= 1.509*10^-2 mol
Step 3: calculate pressure of C2H6
Given:
V = 2.62 L
n = 1.509E-2 mol
T = 34.0 oC
= (34.0+273) K
= 307 K
use:
P * V = n*R*T
P * 2.62 L = 0.0151 mol* 0.08206 atm.L/mol.K * 307 K
P = 0.1451 atm
Answer: 0.145 atm
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