If 0.255 moles of AgNO₃ react with 0.155 moles of H₂SO₄ according to this UNBALANCED equation below, how many grams of Ag₂SO₄ co
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Answer:
Na₂CO₃.2H₂O
Explanation:
For the hydrated compound, let us denote is by Na₂CO₃.xH₂O
The unknown is the value of x which is the amount of water of crystallisation.
Given values:
Starting mass of hydrate i.e Na₂CO₃.xH₂O = 4.31g
Mass after heating (Na₂CO₃) = 3.22g
Mass of the water of crystallisation = (4.31-3.22)g = 1.09g
To determine the integer x, we find the number of moles of the anhydrous Na₂CO₃ and that of the water of crystallisation:
Number of moles =
Molar mass of Na₂CO₃ =[(23x2) + 12 + (16x3)] = 106gmol⁻¹
Molar mass of H₂O = [(1x2) + (16)] = 18gmol⁻¹
Number of moles of Na₂CO₃ = = 0.03mole
Number of moles of H₂O = = 0.06mole
From the obtained number of moles:
Na₂CO₃ H₂O
0.03 0.06
Simplest
Ratio 0.03/0.03 0.03/0.06
1 2
Therefore, x = 2
The volume of a balloon f a gas at 842 mm Hg and -23 celsius if it’s volume is 915 milliliters at a pressure of 1170 mm Hg And a temperature of 24 celsius is 0.22 litres
Explanation:
Data given:
Initial volume of the balloon having gas V1= 915ml OR 0.195 L
initial pressure of the gas P1= 1170 mm Hg OR 1.53 atm
initial temperature of the gas T1 = 24 celsius or 273.15 + 24 = 297.15 K
Final pressure of the gas P2 = 842 mm Hg or 1.10 atm
final temperature of the gas T2 = -23 degrees or 273.15 - 23 = 250.15 K
Final volume at final temperature and pressure V2=?
The formula used is of Gas Law:
=
V2 =
putting the values in the equation:
V2 =
V2 = 0.22 litres is the volume
The volume is 0.22 litres at a pressure of 1170 mmHg and temperature of -23 degrees.