You weighed your empty insulated cup and found that the mass of the cup was 3.1 g.  You add some hot water and find that the total mass increases to 24.9 g.  You got some ice from the bus tub, and found that it was wet.  After drying it carefully, you take the temperature of the hot water in the cup and find that its temperature is 64.8 °C and then add the ice.  The temperature of the water dropped, and came to equilibrium at 33.4 °C.  At the end of the experiment you re-weigh the cup and find that the mass has increased to 30.1 g. What was the initial temperature of the ice?

Consider the following reaction at 37°C. 2 NOCI(g) = 2 NO(g) + Cl₂(g) AG⁰ = 38.5 kJ If 2.17 atm of NOCI are reacted in a rigid container at 37°C, calculate the equilibrium partial pressure (in atm) of NO. atm

Classify each of the reactions according to one of the four reaction types summarized in the table below. Reaction Spontaneous Process? Туре ΔΗ' (system) AS (system) (Standard Conditions) 1 Exothermic, 0 Spontaneous at all temperatures. AS (universe) > 0. Exothermic, 0 Positive, > 0 Depends on relative magnitudes of AH and AS". Spontaneous at higher temperatures. 3 Endothermic, > 0 Negative, < o Not spontaneous at any temperature. AS° (universe) < 0. 4 C6 H12O6 (s) + 6 02 (g) → 6 CO2 (g) + 6 H2O(l) a. A,H° = -673 kJ/mol-rxn A,S° = 60.4 J/K · mol-rxn O Spontaneous at all temperatures. O Spontaneous at lower temperatures. O Spontaneous at higher temperatures. ONot spontaneous at any temperature. b. ВаО(s) + C(graphite) — Ba(s) + СО(g) A,H° = 437.6 kJ/mol-rxn A,S° = 184.9 J/K· mol-rxn OSpontaneous at all temperatures. O Spontaneous at lower temperatures. O Spontaneous at higher temperatures. ONot spontaneous at any temperature.

For the reaction Fe,O3(s) + 3H2(g)–2Fe(s) + 3H,O(g) AH° = 98.8 kJ and AS° = 142.5 J/K %3D The equilibrium constant for this reaction at 345.0 K is Assume that AH° and AS° are independent of temperature.