Please help!! I’m stuck :// Under laboratory conditions, most gases behave like ideal gases because . (Select all that apply). A) at laboratory temperatures and pressures, their interactions are insignificant
B) gas molecules do not have intermolecular forces C) the amount of time molecules interact in the gas phase is small
D) molecules are widely far apart, making intermolecular forces negligible

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

the dissociation of nickel hydroxide is follows:

the concentration of hydroxide ion is

the equilibrium constant value of nickel hydroxide is = 6.1 * 10^-^1^6 and thus equilibrium equation can be written as:

thus, concentration of ni is 0.23 * 10^-^4 mol /l

c. 4.54 x 10–12 j happens to be correct