Cl is stable as a diatomic molecule where the 2 Cl atoms are held together by a covalent bond
molar mass of the diatomic molecule is 70.9 g/mol
therefore 70.9 g of Cl₂ is - 1 mol
then 140 g of Cl₂ is - 1/70.9 x 140 = 1.97 mol
there are 1.97 mol of Cl₂ present
CO₂ + H₂O -------> H₂CO₃
moles of CO₂ =
=
= 11.997 mol
mole ratio of CO₂ : H₂O = 1 : 1
∴ moles of H₂O = (`11.997 mol ) * 1
= 11.997 mol
≈ 12 mol
Answer:
BeCl2 + 2AgNO3 ---> Be(NO3)2 + 2AgCl
Answer:
P₂ = 2.88 atm
Explanation:
Given data:
Initial volume of gas = 1.8 L
Final volume = 750 mL
Initial pressure = 17.5 Psi
Final pressure = ?
Solution:
We will convert the units first:
Initial pressure = 17.5 /14.696 = 1.2 atm
Final volume = 750 mL ×1L/1000L = 0.75 L
The given problem will be solved through the Boly's law,
"The volume of given amount of gas is inversely proportional to its pressure by keeping the temperature and number of moles constant"
Mathematical expression:
P₁V₁ = P₂V₂
P₁ = Initial pressure
V₁ = initial volume
P₂ = final pressure
V₂ = final volume
Now we will put the values in formula,
P₁V₁ = P₂V₂
1.2 atm × 1.8 L = P₂ ×0.75 L
P₂ = 2.16 atm. L/ 0.75 L
P₂ = 2.88 atm
Mass of water added:
0.997 x 1500
= 1495.5 grams
a) Volume = mass / density
Volume = 1495.5 / 0.917
Volume = 1630 cm³ = 1.63 L
b) The ice cannot be contained in the bottle as its volume exceeds that of the bottle.
