Question

Вычислите массу хлорида аммония который образуется при взаимодействии амиака 112 литров с соляной кислотой

Answer 1

NH3 + HCl = NH4Cl

n(HCl) = m(Hcl)/M(HCl) = 7,3/36,5 = 0,2 моль

n(NH3) = 5,1/17 = 0,3 моль

хлороводород в недостатке, он расходуется полностью, по нему и считаем.

n(NH4Cl) = n(HCl) = 0,2 моль

m(NH4CL) = 0,2*53,5 = 10,7 г.

в избытке останется аммиак.

Answer 2

Calculating the Mass of Ammonium Chloride Formed

To calculate the mass of ammonium chloride formed when 112 liters of ammonia reacts with hydrochloric acid, we can use the balanced chemical equation for the reaction between ammonia and hydrochloric acid:

NH3 + HCl → NH4Cl

The balanced equation shows that 1 mole of ammonia reacts with 1 mole of hydrochloric acid to produce 1 mole of ammonium chloride.

Step 1: Convert Liters to Moles

First, we need to convert the volume of ammonia from liters to moles. We can use the ideal gas law to do this:

PV = nRT

Where: - P = pressure (assume standard pressure) - V = volume in liters - n = number of moles - R = ideal gas constant - T = temperature (assume standard temperature)

Step 2: Use Stoichiometry to Find the Mass

Once we have the number of moles of ammonia, we can use the stoichiometry of the balanced chemical equation to find the number of moles of ammonium chloride produced. From there, we can convert the moles of ammonium chloride to grams using the molar mass of ammonium chloride.

Let's proceed with the calculations.

Step 1: Convert Liters to Moles

Using the ideal gas law, we can convert the volume of ammonia to moles. Assuming standard temperature and pressure, the ideal gas constant R is 0.0821 L·atm/mol·K.

Given: - Volume of ammonia (V) = 112 liters - Assume standard temperature and pressure (STP)

We can use the formula PV = nRT to find the number of moles (n) of ammonia.

Step 2: Use Stoichiometry to Find the Mass

Once we have the number of moles of ammonia, we can use the stoichiometry of the balanced chemical equation to find the number of moles of ammonium chloride produced. From there, we can convert the moles of ammonium chloride to grams using the molar mass of ammonium chloride.

Let's proceed with the calculations.