Fluorine and krypton react to form binary compounds when a mixture of the two gases is heated to 500C in a nickel reaction vessel. A 100mL nickel container is filled with fluorin and krypton to partial pressures of 1.24 atm and 10.10 atm, respectively at a room temperature of 20 C. The reaction vessel is heated to 500 C and then cooled to a temperature at which F2 is a gas and krypton fluorides are nonvolatile solids. The remaining F2 gas is transferred to another 100mL nickel container where the pressure of F2 at 20C is 7.2 atm. Assuming all the krypton has reacted, what is the formula of the product?
Check your post. There is something wrong with these numbers or if the numbers are ok you may have transposed the ingredients.
don't have the answer but to help those trying to help, it should be 10.10 atm for Fluorine, and 1.24 atm for Krypton.
I thought that was what happened. The numbers were transposed.
To find the formula of the product, we need to understand the reaction that takes place between fluorine (F2) and krypton (Kr) and use the information provided.
Given:
Partial pressure of F2 before reaction = 1.24 atm
Partial pressure of Kr before reaction = 10.10 atm
Partial pressure of F2 after reaction = 7.2 atm
First, we need to determine the moles of F2 and Kr before the reaction and the moles of F2 after the reaction.
To find the moles of F2 and Kr before the reaction, we will use the ideal gas law:
PV = nRT
Where:
P = pressure
V = volume
n = moles
R = ideal gas constant (0.0821 L * atm / mol * K)
T = temperature (in Kelvin)
Converting the volume to liters and temperature to Kelvin, we have:
Volume = 100 mL = 0.1 L
Temperature before the reaction = 20°C + 273 = 293 K
Using the ideal gas law, we can find the number of moles of F2 and Kr before the reaction.
For F2:
n(F2) = (P(F2) * V) / (R * T)
= (1.24 atm * 0.1 L) / (0.0821 L * atm / mol * K * 293 K)
≈ 0.0526 moles
For Kr:
n(Kr) = (P(Kr) * V) / (R * T)
= (10.10 atm * 0.1 L) / (0.0821 L * atm / mol * K * 293 K)
≈ 0.445 moles
Next, we need to find the moles of F2 after the reaction. Since all the Kr has reacted, the change in moles of F2 is equal to the difference in moles of F2 before and after the reaction.
Change in moles of F2 = n(F2) - n(F2) after reaction
Change in moles of F2 ≈ 0.0526 moles - n(F2) after reaction
Furthermore, the volume of F2 after the reaction is also 100 mL or 0.1 L.
Using the ideal gas law with the pressure of F2 after the reaction, we can find n(F2) after the reaction.
n(F2) after reaction = (P(F2) after reaction * V) / (R * T)
= (7.2 atm * 0.1 L) / (0.0821 L * atm / mol * K * 293 K)
≈ 0.307 moles
Substituting this into the previous equation, we get:
Change in moles of F2 ≈ 0.0526 moles - 0.307 moles
≈ -0.254 moles
Since the moles of F2 have decreased after the reaction by -0.254 moles, we can conclude that the reaction is:
2 F2 + Kr → F2Kr2
Therefore, the formula of the product is F2Kr2, meaning two fluorine atoms are bonded with one krypton atom.