A 0.588 g sample of liquid C5H12 was combusted using excess oxygen gas inside a bomb calorimeter, with the products being carbon dioxide gas and liquid water. The calorimeter's heat capacity is 4.706 kJ °C-1. If the temperature inside the calorimeter increased from 25.0 °C to 29.9 °C, determine ΔrU for this reaction in kJ mol-1 (with respect to C5H12). Do not worry about how realistic the final answer is. Express answer in 2 significant figures.

Use standard enthalpies of formation to calculate ΔH° for the following reaction: SnO2 (s)   +   2 CO (g)   →   Sn (s)   +   2 CO2 (g) The ΔHf° of SnO2 (s) is -907.5 kJ/mol. Be sure to enter a unit with your answer.

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…

A 1.27-g sample of fumaric acid (C4H4O4) is burned in a bomb calorimeter and the temperature increases from 24.70 °C to 27.50 °C. The calorimeter contains 1.01×103 g of water and the bomb has a heat capacity of 755 J/°C. Based on this experiment, calculate ΔE for the combustion reaction per mole of fumaric acid burned (kJ/mol).