1)
Molar mass of H2O2,
MM = 2*MM(H) + 2*MM(O)
= 2*1.008 + 2*16.0
= 34.016 g/mol
mass of H2O2 = 0.11 g
mol of H2O2 = (mass)/(molar mass)
= 0.11/34.02
= 3.234*10^-3 mol
According to balanced equation
mol of O2 formed = (1/2)* moles of H2O2
= (1/2)*3.234*10^-3
= 1.617*10^-3 mol
Given:
V = 2.50 L
n = 1.617*10^-3 mol
T = 298 K
use:
P * V = n*R*T
P * 2.5 L = 0.0016 mol* 0.08206 atm.L/mol.K * 298 K
P = 0.016 atm
Answer: c
2)
Gas is changing to liquid.
So, heat must be released.
So, ΔHo is negative.
Reactant has more entropy than product because of presence of gas in reactant.
So, ΔSo is negative
Answer: d
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