Calculate ΔH and ΔS for the following reaction: NH4NO3(s) + H2O(l) +> NH4+(aq) + NO3-(aq) Use the results of this calculation to determine the value of ΔG° for the reaction at 25°C, and explain why NH4NO3 spontaneously dissolves in water at room temperature

Balance the following redox reaction in an acidic solution: UO22+(aq)+Zn(s)->U4+(aq)+Zn2+(aq)

1. An impure sample of compound A is contaminated with two impurities B and C. The sample is to be purified by recrystallization using ethanol as the solvent. The solubility properties of the three components are summarized below. Solubility in Solubility in ethanol Solubility in 50 mL Solubility in 50 mL ethanol at -78 °C at - 0°C ethanol at -78 °C ethanol at - 0°C (g) (g) Compound A 0.12 g/mL 0.02 g/mL Impurity B 0.58 g/mL 0.04 g/mL Impurity C 0.005 g/mL 0.0003 g/mL The impure (7.5 g) sample contains 5.0 g of compound A, 1.5 g of B and 1.0 g of C and is recrystallized using 50 mL of ethanol. The sample is boiled with 50 mL of ethanol, filtered by gravity and then cooled in ice and filtered by suction. a) How much compound A should be obtained as the final product? Will the sample be contaminated with any of the impurities? Explain (using calculations to support your answer-fill in the missing masses in the table above). Hint: For this question you should calculate the mass of each…

Consider the following reaction in a sealed vessel kept at constant temperature: A(g)  ⇌  2B(g) If the reaction is started with 2.0 mol of A and no B, the amount of B at equilibrium is 3.0 mol. How many moles of A should one start with to obtain 6.0 mol of B at equilibrium under the same conditions (same vessel, same temperature, no gas B present initially)?   A.  5.6 mol   B.  5.0 mol   C.  4.0 mol   D.  6.0 mol   E.  6.5 mol