Calorimetry uses $Q = mc\Delta T$. The $m$ refers to:

Mass of the calorimeter water (or solution) absorbing heat

Enthalpy change for a reaction is the same whether it occurs in one step or multiple, depending only on initial and final states

Bond energies provide an estimate of $\Delta H$ by:

Summing energies of bonds broken (reactants) minus bonds formed (products)

The catalyst in a reaction profile:

Lowers activation energy without changing $\Delta H$

A bomb calorimeter calibration constant $c_{\text{cal}}$ is used because:

The calorimeter itself absorbs heat alongside the contents; the constant captures that

Which is the strongest opening for a VCE Chemistry energetics extended response?

Calculate $Q$ absorbed using $Q = mc\Delta T$, convert to mol of fuel using $n = \frac{m}{M}$, then use $\Delta H = -\frac{Q}{n}$. State the sign convention and significant figures.

§-Quiz

← back to the guide

VCE Chemistry energetics calculations walkthrough quiz

10 questions. Pick an answer and you'll see why right away. Options are shuffled each attempt, and the review at the end links each missed question to the dot point to revise.

An exothermic reaction has enthalpy change $\Delta H$ :
Calorimetry uses $Q = mc\Delta T$ . The $m$ refers to:
Hess's law states:
$\Delta H_{\text{combustion}}$ of methane is $-890$ kJ/mol. The enthalpy change, $\Delta H$ , for burning $0.5$ mol of methane is:
If $200$ mL of water rises from $20.0$ to $28.0$ $^\circ$ C, the heat absorbed is approximately:
Bond energies provide an estimate of $\Delta H$ by:
The catalyst in a reaction profile:
Standard enthalpy of formation $\Delta H_f$ for an element in its standard state is:
A bomb calorimeter calibration constant $c_{\text{cal}}$ is used because:
Which is the strongest opening for a VCE Chemistry energetics extended response?