Answer:
AgNO₃ will be the limiting reagent.
Explanation:
The balanced reaction is:
AgNO₃ + Li → LiNO₃ + Ag
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of each compound participate:
- AgNO₃: 1 mole
- Li: 1 mole
- LiNO₃: 1 mole
- Ag: 1 mole
To determine the limiting reagent, you can use a simple rule of three as follows: if by stoichiometry AgNO₃, how much moles of AgNO₃ will be needed if 0.35 moles of Li react?
moles of AgNO₃= 0.35
But 0.35 moles of AgNO₃ are not available, 0.30 moles are available. Since you have less moles than you need to react with 0.35 moles of Li, <u><em>AgNO₃ will be the limiting reagent.
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Count how many protons there is and search up what symbol has this many protons
The enthalpy : 320.3 kJ/mol
<h3>Further explanation </h3>
The change in enthalpy in the formation of 1 mole of the elements is called enthalpy of formation
The enthalpy of formation measured in standard conditions (25 ° C, 1 atm) is called the standard enthalpy of formation (ΔHf °)
Based on the principle of Hess's Law,
<em>the change in enthalpy of a reaction will be the same even though it is through several stages or ways </em>
Reaction
2Fe (s) + 3Cl₂ (g) → 2FeCl₃ (s) ∆H° = -800.0 kJ/mol x 2
4Fe (s) + 6Cl₂ (g) → 4FeCl₃ (s) ∆H° = -1600.0 kJ/mol
Si(s) + 2 Cl₂ (g) → SiCl₄ (s) ∆H° = -640.1 kJ/mol
Reverse
SiCl₄ (s) → Si(s) + 2 Cl₂ (g) ∆H° = 640.1 kJ/mol x 3
3SiCl₄ (s) → 3Si(s) + 6Cl₂ (g) ∆H° = 1920.3 kJ/mol
------------------------------------------------------------------------ +
3 SiCl₄ (s) + 4 Fe (s) → 4 FeCl₃ (s) + 3 Si (s) ∆H° = 320.3 kJ/mol
The density of an object is mass / volume. These units are unusual but since you are reporting your answer in kg/L, the actual conversion is unnecessary
d = m/V
d = 7.2 kg / 9 L
d = 0.8 kg / L