Enthalpy Change and Calorimetry

In calorimetry, what is directly measured to determine the enthalpy changes of reactions performed at constant pressure?

When two substances at different temperatures are mixed in an isolated calorimeter, what principle dictates the final thermal equilibrium?

How does constant volume calorimetry differ fundamentally from constant pressure calorimetry in measuring thermodynamic properties?

What is the specific heat capacity ($C_s$) a measure of?

If a 50 g piece of metal at 85°C is placed in 100 g of water at 22°C, and the final temperature of the water and metal is 25.6°C, what additional information is needed to calculate the specific heat capacity of the metal?

In a calorimetry experiment, if the calorimeter is not perfectly insulated and some heat is lost to the surroundings, how will this error affect the calculated enthalpy change of the reaction?

In constant pressure calorimetry, if a reaction releases heat, causing the temperature of the water in the calorimeter to increase, what sign is associated with the enthalpy change ($\Delta H$) for the reaction, and why?

If the molar heat capacity ($C_m$) of a substance is given in J/mol·K, how does it relate to the specific heat capacity ($C_s$) of the same substance?

Consider a scenario where 100 mL of 1.0 M HCl is mixed with 100 mL of 1.0 M NaOH in a calorimeter. What primary factor determines the amount of heat released during this neutralization reaction?

In a constant-pressure calorimeter, what is the significance of using a Styrofoam cup as the reaction vessel?

How does increasing the mass of water in a calorimeter affect the measured temperature change for a given amount of heat released by a reaction?

How is the formula $q = mC\Delta T$ applied differently when determining the heat absorbed by a calorimeter itself (as opposed to the solution inside)?

What does Hess's Law state regarding the enthalpy change of a chemical reaction?

According to Hess's Law, if a reaction is reversed, what happens to the sign of the enthalpy change ($\Delta H$)?

When using Hess's Law to calculate the enthalpy change for a target reaction, what mathematical operation is performed on the $\Delta H$ values of the intermediate reactions?

Why is enthalpy considered a state function in the context of Hess's Law?

Consider the following series of reactions: A → B, $\Delta H_1 = -50\text{ kJ}$ and B → C, $\Delta H_2 = -25\text{ kJ}$. According to Hess's Law, what is the enthalpy change for the reaction A → C?

Given that the reaction N2(g) + O2(g) → 2NO(g) has a $\Delta H = +180 \text{ kJ}$, what is the $\Delta H$ for the reaction 2NO(g) → N2(g) + O2(g)?

If you multiply a chemical equation by a factor of 2, what effect does this have on the enthalpy change ($\Delta H$)?

Under what conditions can Hess's Law be most reliably applied to calculate enthalpy changes?

Consider the reactions:

1. A -> B $\Delta H = -30\text{ kJ}$
2. B -> C $\Delta H = +10\text{ kJ}$ What is the enthalpy change for the reaction: A -> C?

Given $\Delta H_f$ [H2O(g)] = -242 kJ/mol and $\Delta H_f$ [H2O(l)] = -286 kJ/mol, what is the enthalpy change for the condensation of water: H2O(g) -> H2O(l)?

Considering these two reactions:

1. C(s) + O2(g) -> CO2(g) $\Delta H = -393.5\text{ kJ}$
2. CO(g) + 1/2 O2(g) -> CO2(g) $\Delta H = -283.0 \text{ kJ}$ what is the enthalpy change for the incomplete combustion of carbon: C(s) + 1/2 O2(g) -> CO(g)?

Given the following thermochemical equations:

C(s) + O2(g) → CO2(g) $\Delta H = -393.5 kJ$ H2(g) + 1/2 O2(g) → H2O(l) $\Delta H = -285.8 kJ$ CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) $\Delta H = -890.3 kJ$

What is the enthalpy of formation of methane, CH4(g)?

What type of process is described when $\Delta H$ is negative?

How does the change in temperature inside a calorimeter relate to the heat exchanged in the reaction?

Given the reaction A + B -> C, (\Delta H) = -50 kJ/mol, what can be concluded?

If Reaction 1: A -> B has (\Delta H_1), and Reaction 2: B -> C has (\Delta H_2), what is the (\Delta H) for the overall reaction A -> C?

What two values must be multiplied together to find the molar heat capacity?

Which equation is used to calculate heat transfer?

In bomb calorimetry, what is directly measured?

When manipulating chemical equations and their respective enthalpy changes per Hess's Law, what must be done if an equation is reversed?

If an equation is multiplied by two, what effect does this have on the enthalpy value?

A reaction produces 100 J of heat that is absorbed by 25 g of water. If the water's initial temperature is 20°C, what is its final temperature, assuming specific heat of water = 4.184 J/g°C?

What is the value of q when a 50.0 g piece of metal at 85.0°C is placed in 100.0 g of water at 22.0°C and the metal and water come to an equilibrium temperature of 25.6°C? (specific heat of water = 4.184 J/g°C)

What is the change in enthalpy, (\Delta H) in kJ, when 50.0 mL of 1.0 M HCl is added to 50.0 mL of 1.0 M NaOH if the temperature increases by 6.5°C? (Assume a total volume of 100 mL, a density of 1.00 g/mL and a specific heat of 4.18 J/g-K.)

What is the term for reactions/processes in which energy is absorbed from the surroundings?

What is the term for reactions/processes in which energy is released into the surroundings?