How many grams of h2so4 are needed to neutralize completely 10 litre of ammonia gas at ntp
First, consider the sulfuric acid a mixture of H2SO4 and water. So the reaction is
2NH3+H2O+H2SO4>>2NH4OH+H2SO4>>(NH4)2SO4+2H2O
so 10 liters of NH3=10/22.4 moles, and it reacts with half that amount, or 5/22.4 mole, so mass of sulfuric acid is 5/22.5 * 98 grams
To determine the amount of H2SO4 needed to neutralize 10 liters of ammonia gas at NTP, we need to know the balanced chemical equation between H2SO4 and ammonia (NH3). Without this information, it is not possible to provide a step-by-step calculation. Could you please provide the balanced chemical equation or any additional information?
To calculate the amount of H2SO4 required to neutralize 10 liters of ammonia gas at NTP (normal temperature and pressure), we need to use stoichiometry. The balanced chemical equation for the neutralization reaction between ammonia (NH3) and sulfuric acid (H2SO4) is:
2 NH3 + H2SO4 -> (NH4)2SO4
In this equation, it shows that 2 moles of NH3 react with 1 mole of H2SO4 to form 1 mole of (NH4)2SO4.
First, we need to calculate the number of moles of NH3 in 10 liters. To do this, we use the ideal gas law, which states:
PV = nRT
Where:
P = pressure (in atmospheres)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
At NTP, the temperature is 273 K and the pressure is 1 atm.
Using the ideal gas law, we can rearrange it to solve for n:
n = PV / RT
Plugging in the values:
n = (1 atm) * (10 L) / (0.0821 L·atm/(mol·K) * 273 K)
Simplifying, we get:
n = 0.452 moles of NH3
Since the reaction is 2 moles of NH3 reacting with 1 mole of H2SO4, we need half the number of moles of H2SO4.
Therefore, the number of moles of H2SO4 needed = 0.452 moles / 2 = 0.226 moles.
Finally, we can convert moles to grams using the molar mass of H2SO4, which is approximately 98 g/mol.
Mass of H2SO4 needed = 0.226 moles * 98 g/mol
So, approximately 22.19 grams of H2SO4 are needed to completely neutralize 10 liters of ammonia gas at NTP.