A reaction has $\Delta H = -90\ \text{kJ mol}^{-1}$. What does this tell you?

It is exothermic and releases heat to the surroundings

In a calorimetry experiment using $q = mc\Delta T$, what must you do to find $\Delta H$ per mole?

Divide $q$ by the number of moles reacting

Bonds broken minus bonds formed

Hydrogen bonds hold the molecules in an open lattice with larger spacing

The area under the curve equals the total number of molecules

It speeds up the forward and reverse reactions equally, so equilibrium is reached faster but the position is unchanged

Hot ethanolic (alcoholic) hydroxide

10questions. Pick an answer and you'll see why right away.

A reaction has $\Delta H = -90\ \text{kJ mol}^{-1}$ . What does this tell you?
In a calorimetry experiment using $q = mc\Delta T$ , what must you do to find $\Delta H$ per mole?
Using mean bond enthalpies, how is $\Delta H$ for a reaction calculated?
Which intermolecular force is present between all molecules?
Why is ice less dense than liquid water?
Which key feature of the Maxwell-Boltzmann distribution is correct?
What is the only factor that changes the value of the equilibrium constant $K_c$ ?
How does adding a catalyst affect a system at equilibrium?
What is formed when a secondary alcohol is oxidised with acidified potassium dichromate?
Which conditions favour elimination rather than substitution when a haloalkane reacts with hydroxide?