Question

Consider the following gas phase reaction: 12(g) + Cl2(g) →21C1(e) If 4.46 liters of Cl(s) gas at 119°C and 0.996 atm is used, what volume of ICl(g) gas will be formed if it is collected at 168°C and 1.21 atm? liters Submit Answer Retry Entire Group 1 more group attempt remaining

Answer 1

1st calculate mol of Cl2

Given:

P = 0.996 atm

V = 4.46 L

T = 119.0 oC

= (119.0+273) K

= 392 K

find number of moles using:

P * V = n*R*T

0.996 atm * 4.46 L = n * 0.08206 atm.L/mol.K * 392 K

n = 0.1381 mol

From reaction,

Mol of ICl formed = 2*mol of Cl2 reacted

= 2*0.1381 mol

= 0.2762 mol

Given:

P = 1.21 atm

n = 0.2762 mol

T = 168.0 oC

= (168.0+273) K

= 441 K

use:

P * V = n*R*T

1.21 atm * V = 0.2762 mol* 0.08206 atm.L/mol.K * 441 K

V = 8.2605 L

Answer: 8.26 L