Consider the combustion of liquid C5H in oxygen gas to produce carbon dioxide gas and water vapor. In an experiment, 0.1063 g of C;Hg is combusted to produce enough heat to raise the temperature of 150.0 g of water by 7.632 °C. Write the reaction that takes place using whole number coefficients.

The combustion of 0.1584 grams of benzoic acid increases the temperature of a calorimeter by 2.54 C. Calculate the heat capacity of this calorimeter. The energy released by the combustion of benzoic acid is 26.42 kJ/gram.

Write and balance the equation for the complete combustion of heptane, C7H16.C7⁢H16. Phase symbols and energy changes are optional.

A 1.00 g sample of NH4NO3 is decomposed in a bomb calorimeter.  The temperature of the calorimeter increases by 6.12 K.  The heat capacity of the system is 1.23 kJ/g·K.  What is the molar heat of decomposition for ammonium nitrate?

In a coffee-cup calorimeter, 1.59 g NH4NO3 is mixed with 74.3 g water at an initial temperature of 25.45°C. After dissolution of the salt, the final temperature of the calorimeter contents is 23.25°C. Assuming the solution has a heat capacity of 4.18 J/°C·g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol. ΔH =  kJ/mol

Section 5.6 You place 0.0750 g of magnesium chips in a coffee-cup calorimeter and then add 100.0 mL of 1.00 M HCI. The reaction that occurs is: -> Mg (s) + 2 HCI (aq) → H2 (g) + MgCl2 (aq) The temperature of the solution raises from 20.15 °C to 23.29 °C. What is the enthalpy change or the reaction per mole of Mg? Assume that the specific heat capacity of the solution is 4.20 J/g K and the density of the solution is 1.00 g/mL. 412 kJ/mol 428 kJ/mol -412 kJ/mol -428 kJ/mol

A 0.602-g sample of isophthalic acid (C8H604) is burned in a bomb calorimeter and the temperature increases from 24.80 °C to 27.05 °C. The calorimeter contains 1.01x10³ g of water and the bomb has a heat capacity of 936 1/°C. The heat capacity of water is 4.1843 g ¹¹. Based on this experiment, calculate AE for the combustion reaction per mole of isophthalic acid burned. 9 kJ/mol

For the highly exothermic reaction H2(g) + 1/2 O2(g) → H2O(g) qrx =DHrx = -242 kJ, What quantity of heat (kJ) is exchanged when 17.9 moles of hydrogen and 1.13 moles of oxygen are combusted?

When a 8.00 g sample of KCN is dissolved in water in a calorimeter that has a total heat capacity of 2.93 kJ⋅K−1, the temperature decreases by 0.490 K. Calculate the molar heat of solution of KCN.

A calorimeter is calibrated by mixing two aqueous solutions each with a volume equal to 44.4 mL. The reaction is known to produce 1,465 J of heat, and the measured temperature rise is 4.64 K. Heat produced by the reaction is absorbed by the calorimeter and the resulting solution in it. The same calorimeter is used in a subsequent experiment where 44.4 mL of 0.430 mol L-1 HCl are mixed with 44.4 mL of 0.43 of NaOH. The temperature rises by 3.38. Calculate the heat evolved by the reacting system in J *be sure to include the correct sign in your answer*. heat evolved (J) = What is the enthalpy of the neutralization reaction in kJ/mol ? Enthalpy of Reaction (kJ/mol) = kJ/mol