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1.00atm of H2 and 1.00atm of Br2 were mixed in a 1.00L flask at 25°C. Under...

1.00atm of H2 and 1.00atm of Br2 were mixed in a 1.00L flask at 25°C. Under the appropriate conditions, gaseous HBr will form. At equilibrium, 1.10×10^13 molecules of H2 were found. Given the information below, calculate the values of K, delta G°, and delta S°. (for this problem, you do not have available values of free energies of formation and values of entropies of formation.)
H2(g) + Br2(g) ----> 2HBr(g)   delta H°= -103.8kJ

Solutions

Expert Solution

first to calculate Molarity.

using the ICE table to determine the concentration of all at equilibrium.

then to find Kc.

then ∆G°

then to find ∆S°

queen_honey_blossom answered 8 months ago
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