Consider the following equilibrium: HC2O4- + HSO4- <—> H2C2O4 + SO42-
The order of Bronsted-Lowry acids and bases in the reaction is .

See explanation

Explanation:

According to Bronsted-Lowry definition of acids/bases, an acid is a proton donor while a base is a proton acceptor.

Hence, in a reaction, the species that donate protons are strong acids while the species that accept protons are strong bases.

Hence, HSO4- is a stronger acid than H2C2O4 and SO42- is a weaker base than HC2O4-

Note that the conjugate base of a strong acid is a weak base and vice versa.

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