1- What volume of hydrogen gas at 273 K and 1 atm pressure will consumed in obtaining 2.16 gm of elemental born(atomic mass=10.8)from the reduction of born trichloride by hydrogen:
A- 44.8 lit B-22.4 lit C- 89.6 lit D-67.2 lit
B
22.4lt
To calculate the volume of hydrogen gas consumed in the given reaction, we need to use the ideal gas law equation, which is:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
First, we need to calculate the number of moles of elemental boron (B):
Given mass of elemental boron = 2.16 g
Atomic mass of boron = 10.8 g/mol
n = (mass) / (atomic mass)
n = 2.16 g / 10.8 g/mol
n = 0.2 mol
Since the reaction equation is not provided, I will assume it is balanced and that all three chlorine atoms are replaced by three hydrogen atoms when reducing boron trichloride (BCl3) to elemental boron (B).
From the balanced equation, we can determine the stoichiometry between boron trichloride (BCl3) and hydrogen (H2). Assuming one mole of BCl3 requires three moles of H2 for the reaction:
n(BCl3) = n(H2)/3
n(H2) = 3 * n(BCl3)
n(H2) = 3 * 0.2 mol
n(H2) = 0.6 mol
Now we can substitute the values into the ideal gas law equation:
PV = nRT
P * V = n * R * T
V = (n * R * T) / P
V = (0.6 mol * 0.0821 L·atm/(mol·K) * 273 K) / 1 atm
V = 11.24 L
Therefore, the volume of hydrogen gas consumed is approximately 11.24 liters.
None of the options listed (A, B, C, D) match the calculated value, so there may be an error in the provided options, or the question may be incorrect.