Answer:
See explanation
Explanation:
Number of moles of Cl2 = 0.71g/71g/mol = 0.01 moles
Number of moles = 1.0 g/38g/mol = 0.02 moles
Total = 0.01 + 0.02 = 0.03 moles
From the ideal gas equation;
PV=nRT
P=?
V= 258 ml
n= 0.03 moles
T= 296 K
P= nRT/ V
P= 0.03 × 0.082 × 296/258
P= 0.003 atm
Partial pressure Cl2 = 0.01/0.03 × 0.003 atm = 0.001 atm
Partial pressure = F2 = 0.02/0.03 × 0.003atm = 0.002 atm
