Answer:
0.488 mol
Explanation:
By the ideal gas law:
PV = nRT
Where P is the pressure, V is the volume, n is the number of moles, R is the gas constant (0.082 atm.L/mol.K), and T is the temperature in K. Thus, after the reaction:
P = 2.92 atm
V = 4.50 L
T = 55.2°C + 273 = 328.2 K
PV = nRT
n = PV/RT
n = (2.92*4.50)/(0.082*328.2)
n = 0.488 mol
By an IUPAC definition, solvation is an interaction of a solute with the solvent, which leads to stabilization of the solute species in the solution. In the solvated state, an ion in a solution is surrounded or complexed by solvent molecules. ... Solvation or dissolution is a kinetic process and is quantified by its rate.
That illustration represents the mitochondria
Redox
reactions are those in which the oxidation numbers of the elements involved are
changed.
Equation
1:
2Na(s)
+ Cl2(g) --> 2NaCl
The
oxidation numbers of Na and Cl in the reactant side are both zero because they
are in elemental form. In the product side, however, the oxidation numbers are
+1 and -1, respectively. Hence, this is an example of redox reaction.
Equation
2:
Cd(s)
+ Pb+2(aq) --> Cd2+(aq) + Pb(s)
The
oxidation numbers of Cd and Pb+2 in the reactant side are 0 and +2,
respectively. They are, however, +2 and 0 in the product side. Hence, this is
also a redox reaction.
Equation
3:
Pb(NO3)2(liq)
+ 2LiCl(aq) --> PbCl2(s) + 2LiNO3(aq)
The
oxidation numbers of the involved ions (both cations and anions) are not
changed. Hence, this is NOT an oxidation reaction.
Equation
4:
C(s)
+ O2(g) --> CO2(g)
Just
as the equation 1 and 2, the oxidation numbers of the reactants are not similar
to those in the product. Hence, this is an example of oxidation reaction.
Answer:
6.18 g
Explanation:
We know we will need a balanced equation with masses, moles, and molar masses, so let’s gather all the information in one place.
: 41.99
Na₂SiO₃ + 8HF ⟶ 2NaF + H₂SiF₆ + 3H₂O
<em>n</em>/mol: 0.58
1. Use the molar ratio of NaF:HF to calculate the moles of NaF.
2. Use the molar mass of NaF to calculate the mass of NaF.
