Ni+4CO=NI(CO)4
this reaction separates nickel from other solid impurities.Starting with 86.4g NI,calculte the pressure of NI(CO)4 in a container of volume 4.00L
Convert 86.4 g Ni to moles(moles = g/molar mass), using the coefficients in the balanced equation convert moles Ni to moles Ni(CO)4, then use PV = nRT to determine pressure.
To calculate the pressure of NI(CO)4 in the container, we need to use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
First, we need to determine the number of moles of NI(CO)4 that are produced from 86.4g of nickel. We can use the molar mass of nickel to convert grams to moles. The molar mass of nickel is approximately 58.69 g/mol.
Moles of NI = Mass of NI / Molar mass of NI
Moles of NI = 86.4 g / 58.69 g/mol
Moles of NI = 1.473 mol
From the balanced equation, we can see that 1 mole of Ni reacts with 4 moles of CO to produce 1 mole of NI(CO)4. Therefore, the number of moles of NI(CO)4 produced is also 1.473 mol.
Now we can substitute the values into the ideal gas law equation to calculate the pressure:
PV = nRT
P * 4.00 L = 1.473 mol * 0.0821 atm L/mol K * T
P = (1.473 mol * 0.0821 atm L/mol K * T) / 4.00 L
To calculate the pressure, we need to know the temperature (T) of the container.