Determine the ΔUoreaction at 25 °C (in kJ/mol) for the following reaction: 5PbO2(s) + 4P(s, white)→P4O10(s) + 5Pb(s)

A student dissolves 13.2 g of sodium hydroxide (NaOH)in 300. g of water in a well-insulated open cup. She then observes the temperature of the water rise from 21.0 °C to 33.4 °C over the course of 5.3 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: + NaOH (s) — Na" (ад) + ОН (ад) olo You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to 3 significant digits. Ar Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. exothermic x10 Is this reaction exothermic, endothermic, or neither? endothermic neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. kJ kJ Calculate the…

3. Calculate the value of ΔSo for the formation of POCl3 from its constituent elements, as shown below. P2(g) + O2(g) + 3Cl2(g) → 2POCl3(g)

Consider the reaction: 2 H,0(g) → 2H,(g) + 0,(g) If 2.0 moles of H2O(g) are converted to H2(g) and 02(g) against a pressure of 1.0 atm at 125 °C, what is the change in internal energy for this reaction? R-8.314 1/mol K AH- 483.6 kl/mol

Calculate AS°rxn for the following reaction. The S° for each species is shown below the reaction. N2H4(l) + H2(g) → 2 NH3(g) ings S°(J/(mol·K)) 121.2 130.7 192.8 O -59.1 J/K es O 311.0 J/K O 133.7 J/K O -133.7 J/K O 637.5 J/K

When 2.53 g of CaCl2 was dissolved in 30.00 g of water in an adiabatic calorimeter at 23.0°C, the temperature of the solution went up to 36.5°C. Find ΔH (in kJ/mol) for the dissolution of one mole of CaCl2 in water. (The molar mass of CaCl2 is 110.978 g/mol.)

A mixture of CO(g) and H2(g) is produced by passing steam over hot charcoal: H2O(g)+ C(s)->H2(g)+CO(g) Using the appropriate thermodynamic values in the table below, calculate the lowest temperature at which the reaction is spontaneous under standard conditions. Compound ΔGf (kJ/mol) ΔHf (kJ/mol) ΔHf (kJ/mol) H2O(g) –228.6 –241.8 188.8 H2O(ℓ) –237.2 –285.8 69.9 C(s) 0.0 0.0 5.7 H2(g) 0.0 0.0 130.6 CO(g) –137.2 –110.5 197.7 O2(g) 0.0 0.0 205.0 _____K

25°C 32°C bum wohl 891 10 228 1. Two aqueous reactants are mixed in a flask with a balloon over the top and the following change is observed. What are the signs on q and w for the system? Enter >, <, or in each box below. W 0 2. You drop a piece of potassium metal into water and the following exothermic reaction occurs: 2 K(s) + 2 H₂O(l) → 2 KOH(aq) + H₂(g) What are the signs on q and w for this reaction, at constant temperature and pressure? A) q is positive and w is negative. B) q is negative and w is positive. C) q and w are both negative. D) q and w are both positive. E) There is not enough information given. 3. What is the change in internal energy when one mole of helium gas in a flexible-walled container at STP is heated to 100°C? (CHe(g) = 5.30 J/g°C) AU =

Consider the reaction that happens at -13 °C: 1A + 2B 8C + 6D. Using the data from the table: B C D AH; (kJ mol 1) 309 144.4 149.5 s° (U mol 1 K1) 61.4 33.6 76.4 153.4 calculate AG° (in kJ) of the reaction. (assume that values of AH and S do not change with the temperature) Enter a number with sign (+ or -) to 1 decimal place in kJ.

Consider the following reaction: Sr(OH)2(s) → Sr2+(aq) + 2 OH-(aq)     ΔHorxn = -19.3 kJ/ mol Sorxn = -218.3 J/ K mol Which of the following statements is true? Group of answer choices: - the reaction is always non-spontaneous - The reaction is nonspontaneous at all temperatures - The reaction is spontaneous only at high temperature - The reaction is spontaneous only at low temperature - ΔG < 0 and the reaction is always spontaneous