The equilibrium constant for the reaction below is 7.2 10-4 at ...

[natalie2426]

Question 1

The enthalpy change for converting 10.0 g of ice at -25.0 °C to water at 80.0 °C is ________ kJ. The specific heats of ice, water, and steam are and respectively. For H₂O, = 6.01 kJ mol^-1, and .
◦ 12.28
◦ 6.16
◦ 3870
◦ 7.21
◦ 9.88

Question 2

The equilibrium constant for the reaction below is 7.2 × 10^-4 at 298 K and 1 atm.

HNO₂(aq) + H₂O(l) NO₂^-(aq) + H₃O⁺(aq)

When [HNO₂(aq)] = 1.0 M and [NO₂^-(aq)] = [H₃O⁺(aq)] = 1.0 × 10^-5 M, calculate ΔG.
◦ -39.1 kJ/mol
◦ +17.9 kJ/mol
◦ -17.9 kJ/mol
◦ +39.1 kJ/mol
◦ -23.02 kJ/mol

[upturnedfurball]

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