Answer:
2.64 × 10⁶ g
Explanation:
We can find the mass of air using the ideal gas equation.

where,
P is the pressure (P = 1.00 atm)
V is the volume (V = 2.95 × 10⁶ L)
n is the number of moles
R is the ideal gas constant (0.08206atm.L/mol.K)
T is the absolute temperature (121°C + 273 = 394 K)
m is the mass
M is the molar mass (28.09 g/mol)

Answer:
The attractive force is negative and MgO has a higher melting point
Explanation:
From Couloumb's law:
Energy of interaction, E = k 
where q1 and q2 are the charges of the ions, k is Coulomb's constant and r is the distance between both ions, i.e the atomic radii of the ions.
If you look at Coulomb's law, you note that in the force is negative (because q1 is negative while q2 is positive).
In addition to that, the compounds MgO and NaF have similar combined ionic radii, then we can determine the melting point trend from the amount of energy gotten
The melting point of ionic compounds is determined by 1. charge on the ions 2. size of ions. while NaF has smaller charges (+1 and -1), MgO (+2 and -2) has larger charges and greater combined atomic radii. This implies that the compound with greater force would have a higher melting point.
Hence the compound MgO would have a higher melting point than NaF.
The equation of the reaction is:
Na2CO3 + AgNO3 → NaNO3 + Ag2CO3
but this equation, not a balanced equation so let's make it a balanced equation:
- we will start with Na number of atoms, we should make the Na atom number is equal on both sides.So we put 2 NaNO3 instead of NaNO3
- and then the Ag atom, we put 2AgNO3 instead of AgNO3 to make the number of Ag on each side are equals.
So the final balanced equation for this reaction is:
Na2CO3(aq) + 2AgNO3(aq) → 2NaNO3(aq) + Ag2CO3(s)
SO know we have number of Na on each side = 2
number of Ag on each side = 2
The unbalanced equation is:
Fe(s) + O2(g) —> Fe2O3(s)
To balance oxygens, multiply O2 by 3 and Fe2O3 by 2.
Fe(s) + 3O2(g) —> 2Fe2O3(s)
Balance your iron by multiplying Fe by 4, since you have 4 Fe in the products now.
4Fe(s) + 3O2(g) —> 2Fe2O3(s)