Chemistry 12: Thermochemistry

Given the reaction $2 C_4H_{10}(g) + 13 O_2(g) \rightarrow 8 CO_2(g) + 10 H_2O(g) + 5314.6 \text{ kJ}$, what is the molar enthalpy change for the combustion of butane gas?

Which of the following correctly pairs the type of energy change that occurs during propane combustion with its cause?

A $50.0 \text{ g}$ block of copper at $10.0 \text{°C}$ is carefully lowered into $100.0 \text{ g}$ of water at $90.0 \text{°C}$ in an insulated container. Which equation, based on the first law of thermodynamics, should be used to calculate the heat transfer in this system?

What is the total amount of heat transferred by $100.0 \text{ g}$ of water when the temperature of the water is increased from $30.0 \text{°C}$ to $45.0 \text{°C}$? (Given: $c_{\text{water}} = 4.184 \text{ J/g°C}$)

Given the following reactions and their enthalpy changes:

$2 C_3H_6(g) + 9 O_2(g) \rightarrow 6 CO_2(g) + 6 H_2O(l) \quad \Delta H^\circ = -3918.4 \text{ kJ}$ $C(s) + O_2(g) \rightarrow CO_2(g) \quad \Delta H^\circ = -393.5 \text{ kJ}$ $H_2(g) + \frac{1}{2} O_2(g) \rightarrow H_2O(l) \quad \Delta H^\circ = -285.8 \text{ kJ}$

What is the molar enthalpy of formation of cyclopropane, $C_3H_6(g)$?

A student dissolves $1.68 \text{ g}$ of ammonium nitrate ($NH_4NO_3$) in $150.0 \text{ g}$ of water in a simple calorimeter. The initial temperature of the calorimeter and contents is $22.30 \text{°C}$, and the final temperature is $20.98 \text{°C}$. Based on this data, what is the molar enthalpy of solution for ammonium nitrate?

Given the reaction $2 H_2O(l) + 571.6 \text{ kJ} \rightarrow 2 H_2(g) + O_2(g)$, what mass of water can be decomposed with the addition of $800.0 \text{ kJ}$ of energy?

A $75.0 \text{ g}$ chocolate mini roll contains $1213.4 \text{ J}$. If walking expends $810 \text{ kJ/h}$, how long would a student have to walk to burn off the energy from three of these mini rolls?

Which substance has a molar enthalpy of formation ($\Delta H_f$) equal to $0.0 \text{ kJ/mol}$?

A reaction of a small amount of material results in a large increase in the temperature of the water in a calorimeter. Which statement accurately describes the $\Delta H$ for the reaction?

Which energy change occurs in water when it is heated from $25.0 \text{°C}$ to $50.0 \text{°C}$?

Given the molar mass of a substance and the information provided in a heating curve graph, showing temperature versus time, what additional information is needed to calculate the energy required to heat $11.2 \text{ g}$ of the compound from point X (solid phase) to point Y (liquid phase)?

It was determined that adding $50.0 \text{ kJ}$ of energy to a calorimeter causes an increase in temperature of $2.50 \text{°C}$. What is the energy change of a reaction, taking place in the calorimeter, if the reaction causes a temperature increase of $7.50 \text{°C}$?

What is the mass of a piece of aluminum if it requires $3.00 \text{ kJ}$ of energy to raise its temperature by $115 \text{°C}$? (Note: $c_{Al} = 0.90 \text{ J/g°C}$)

Using the data below, what is the $\Delta H^\circ$ for the following reaction?

$CH_4(g) + 2 O_2(g) \rightarrow CO_2(g) + 2 H_2O(g)$

Given: $\Delta H_f^\circ CH_4(g) = -75 \text{ kJ/mol}$ $\Delta H_f^\circ CO_2(g) = -390 \text{ kJ/mol}$ $\Delta H_f^\circ H_2O(g) = -240 \text{ kJ/mol}$

Using the average bond energies provided, estimate the enthalpy change ($\Delta H$) for the following reaction:

$2 C_3H_6 (g) + 9 O_2 (g) \rightarrow 6 CO_2 (g) + 6 H_2O (g)$

(Average Bond Energies in kJ/mol: C-C = 347, C=C = 607, C-H = 338, O=O = 498, C=O = 745, O-H = 460)

5.50 g of $NaOH(s)$ reacts with 175 mL of 0.550 mol/L $HCl(aq)$ in a coffee cup calorimeter. If the temperature of the water increased by $2.1°C$, what calculation is needed to determine the molar enthalpy change of the acid?

Using the data below, calculate the enthalpy change for the following reaction: $C_2H_4(g) + 6 F_2(g) \rightarrow 2 CF_4(g) + 4 HF(g)$ given the listed enthalpies.