solution:
First we calculate the number of mole of gas as follows:
PV = n RT
Here temperature; T= 100°C or 373 K
n = PV/ RT
= 4.78 atm * 3.82 L / 0.0821 L ∙ atm / mol ∙ K * 373 K
= 0.596 Moles
Now determine the molar mass of gas as follows:
Number of moles = amount in g/ molar mass
Molar mass = 19.08 grams / 0.596 Moles
= 32.013 g/ mole
This the molar mass of O2 hence the gas is oxygen
First we need to find the number of moles of hydrogen gas formed
Zn + 2HCl ---> ZnCl₂ + H₂
stoichiometry of Zn to H₂ is 1:1
the number of Zn moles reacted - 2.4 g / 65.4 g/mol = 0.0367 mol
assuming Zn to be the limiting reactant
number of Zn moles reacted = number of H₂ moles formed
therefore number of H₂ moles formed = 0.0367 mol
we can use ideal gas law equation to find the pressure
PV = nRT
P - pressure
V - Volume - 450 x 10⁻⁶ m³
n - number of moles - 0.0367 mol
R - universal gas constant - 8.314 Jmol⁻¹K⁻¹
T - temperature - 32 °C + 273 = 305 K
substituting these values in the equation
P x 450 x 10⁻⁶ m³ = 0.0367 mol x 8.314 Jmol⁻¹K⁻¹ x 305 K
P = 206.8 kPa
pressure is 206.8 kPa
Answer:
Hydrogen and chlorine need to be balanced. There is an equal amount of magnesium on each side.
Explanation:
The given chemical equation does not hold the law of conservation of mass because the number of atoms of hydrogen and chlorine are not balanced on each side.
Chemical equation:
Mg + HCl → MgCl₂ + H₂
Balanced chemical equation:
Mg + 2HCl → MgCl₂ + H₂
Now this equation hold the law of conservation of mass.
Law of conservation of mass:
According to the law of conservation mass, mass can neither be created nor destroyed in a chemical equation.
Explanation:
This law was given by french chemist Antoine Lavoisier in 1789. According to this law mass of reactant and mass of product must be equal, because masses are not created or destroyed in a chemical reaction.
You are looking at a decomposition reaction because the original compound is being broken into its individual elements.<span />