Answer:
2.0 × 10⁻³ g
Explanation:
Step 1: Given data
- Mass of solution: 1000. g (1.000 kg)
- Concentration of Br₂: 2.0 ppm
Step 2: Calculate the mass of Br₂ required to prepare the solution
The concentration of Br₂ is 2.0 ppm, that is, there are 2.0 mg of Br₂ per kilogram of solution. The mass of Br₂ required to prepare 1.000 kg of solution is:
1.000 kg Solution × 2.0 mg Br₂/1 kg Solution = 2.0 mg
Step 3: Convert the mass to grams
We will use the conversion factor 1 g = 1000 mg.
2.0 mg × 1 g/1000 mg = 2.0 × 10⁻³ g
Answer:
Density of Radon is 5.44 g/.
Explanation:
Given data:
Temperature of gas = 100°C (273+100 = 373 K)
Pressure of gas = 0.75 atm
Density of gas = ?
Solution:
First of all we will derive the formula.
We know that,
PV = nRT
and
n = m/M (m = mass, M = molar mass)
PV = (m/M) RT
PVM = (m/M) RT ×M
PVM = mRT
PVM/V = mRT/V
PM = dRT (m/V = d)
Now we will put the values in formula:
Molar mass of Radon is 222 g/mol .
0.75 atm ×222 g/mol = d× 0.0821 atm.L/mol.K ×373 K
166.5 atm.g/mol = d×30.62 atm.L/mol
d = 166.5 atm.g/mol / 30.62 atm.L/mol
d = 5.44 g/L
