Question

assume you mix 0.71g of chlorine with 1.00g of fluorine in a 258 ml flask at 23 . what is the partial pressure of each gas

Answer 1

See explanation

Step-by-step 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