<u>Answer:</u> The formula of the compound formed between rubidium and fluorine is RbF
<u>Explanation:</u>
Ionic bond is defined as the bond which is formed by complete transfer of electrons from one atom to another atom.
The atom which looses the electron is known as electropositive atom and the atom which gains the electron is known as electronegative atom. This bond is usually formed between a metal and a non-metal.
Rubidium is the 37th element of the periodic table having electronic configuration of 
This will loose 1 electron to form 
ion
Fluoride is the 9th element of the periodic table having electronic configuration of 
This will gain 1 electron to form 
ion
To form 
compound, 1 rubidium ion is needed to neutralize the charge on fluoride ion
The formation of the given compounds is shown in the image below.
Answer:
Cobaltous Nitride,I think so anyway.......
the balanced chemical equation for the reaction is as follows
H₃PO₄ + 3KOH ---> K₃PO₄ + 3H₂O
stoichiometry of H₃PO₄ to KOH is 1:3
first we have to find which the limiiting reactant is
as the amount of product formed depends on the amount of limiting reactant present
number of H₃PO₄ moles reacted - 4.4 mol
if H₃PO₄ is the limiting reactant
1 mol of H₃PO₄ reacts with 3 mol of KOH
then 4.4 mol of H₃PO₄ reacts with - 3 x 4.4 mol = 13.2 mol of KOH
but only 3.8 mol of KOH is present
therefore KOH is the limiting reactant
stoichiometry of KOH to K₃PO₄ is 3:1
number of KOH moles reacted - 3.8 mol
therefore number of K₃PO₄ formed = number of KOH moles reacted / 3
= 3.8 mol / 3 = 1.3 mol
answer is 1.3 mol of K₃PO₄
Taking into accoun the STP conditions and the ideal gas law, the correct answer is option e. 63 grams of O₂ are present in 44.1 L of O2 at STP.
First of all, the STP conditions refer to the standard temperature and pressure, where the values used are: pressure at 1 atmosphere and temperature at 0°C. These values are reference values for gases.
On the other side, the pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:
P×V = n×R×T
where:
- P is the gas pressure.
- V is the volume that occupies.
- T is its temperature.
- R is the ideal gas constant. The universal constant of ideal gases R has the same value for all gaseous substances.
- n is the number of moles of the gas.
Then, in this case:
- P= 1 atm
- V= 44.1 L
- n= ?
- R= 0.082
- T= 0°C =273 K
Replacing in the expression for the ideal gas law:
1 atm× 44.1 L= n× 0.082 × 273 K
Solving:
n=1.97 moles
Being the molar mass of O₂, that is, the mass of one mole of the compound, 32 g/mole, the amount of mass that 1.97 moles contains can be calculated as:
= 63.04 g ≈ <u><em>63 g</em></u>
Finally, the correct answer is option e. 63 grams of O₂ are present in 44.1 L of O2 at STP.
Learn more about the ideal gas law:
The answer to question 8 is
Ethanol's Molar Heat of Combustion. ... Heats of combustion are quoted as positive numbers while the enthalpy changes of combustion reactions (ΔH) are quoted as negative numbers, as combustion reactions are always exothermic. Heats of combustion are typically stated in kilojoules per mole (kJ/mol. or kJ mol. -1).
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