What volume of ammonia gas at STP is required to neutralise 40cm of 2m sulphuric acid
Note that 2m H2SO4 means 2 molAL. I am almost certain that you mean 2M which is 2 molAR. I will assume the latter.
......H2SO4 + 2NH3 ==> (NH4)2SO4
mols H2SO4 = M x L = ?
mols NH3 = twice mols H2SO4
Convert mols NH3 to volume using PV = nRT
Post your work if you get stuck.
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What you mean by
PV=nRT
To find out the volume of ammonia gas required to neutralize 40 cm³ of 2M sulfuric acid at STP (Standard Temperature and Pressure), we need to use the balanced chemical equation for the reaction between ammonia and sulfuric acid.
The balanced chemical equation is:
2NH₃ + H₂SO₄ → (NH₄)₂SO₄
From the balanced equation, we can see that two moles of ammonia (NH₃) are required to neutralize one mole of sulfuric acid (H₂SO₄).
Step 1: Calculate the moles of sulfuric acid:
Given that the volume of sulfuric acid is 40 cm³ and the concentration is 2M (moles per liter), we can calculate the number of moles of sulfuric acid (H₂SO₄) using the formula:
Moles = Volume x Concentration (in liters)
Moles = (40 cm³ / 1000) x 2M
Step 2: Determine the volume of ammonia gas:
Since two moles of ammonia (NH₃) are required to neutralize one mole of sulfuric acid (H₂SO₄), the volume of ammonia gas will also be two times the volume of sulfuric acid.
Therefore, the volume of ammonia gas required is:
Volume of ammonia gas = 2 x (40 cm³ / 1000)
Finally, convert the volume of ammonia gas to the appropriate units (if necessary).
Note: STP conditions are defined as a temperature of 0°C (273 K) and a pressure of 1 atmosphere. These conditions will need to be taken into account for more accurate calculations.