energy

A sample of silver with a mass of 1.00 g increases in temperature from 20.00°C to 28.00°C. Given that silver has a specific heat of 0.235 J/(g⋅°C), the quantity of heat absorbed is

1.88

How much heat is absorbed by a 10.0 g sample of iron when its temperature increases by 10.0∘C? The specific heat of iron is 0.449 J/(g⋅∘C).

44.9 J

Place these steps in order so that they describe how a calorimeter is used to measure energy that is absorbed or released

A known mass of water is placed in an insulated chamber. The initial temperature of the water is recorded. The reaction takes place and either releases energy to the water or absorbs energy from the water. The water cools down or heats up accordingly. The final temperature of the water is recorded.

Which statements about how a calorimeter is used to measure energy that is absorbed or released are true?

The data to be collected is the change in temperature of the water. Water absorbs the energy released in the reaction, or releases the energy absorbed by the reaction. It is important that the mass of water used be known.

Which statements about kinetic and potential energy are correct?

The potential energy of a substance depends on its composition. The kinetic energy of a substance is proportional to temperature. Chemical systems contain both kinetic energy and potential energy.

Heat flows from the surroundings to the system when a(n) ____ reaction takes place.

endothermic

The heat content of a system at constant pressure is its___

enthalpy

Which is the term for the change in enthalpy for a reaction?

enthalpy of reaction

The sign of enthalpy changes for ________ reactions is always negative.

exothermic

What are the two basic forms in which energy exists?

potential energy kinetic energy

Energy due to the composition or position of an object is _____ energy, while energy of motion is _____

potential; kinetic

Which is the correct expression of the equation for calculating heat?

q = m × c × ΔT

The specific heat of a substance is the amount of heat required to ______.

raise the temperature of one gram of the substance by one degree Celsius

The quantity of heat absorbed or released by a substance is equal to the product of its_______ heat, the ________ of the substance, and the change in its______ .

specific; mass; temperature

In thermochemistry, the specific part of the universe that contains the reaction or process you wish to study is the_____

system

During an exothermic reaction, heat flows from the ______.

system to the surroundings

During an exothermic reaction, heat flows from the_______

system to the surroundings

In thermochemistry, which is the specific part of the universe that contains the reaction or process you wish to study?

the system

In thermochemistry, the system plus the surroundings is the____

universe

Which equation correctly shows how the enthalpy of reaction is related to the enthalpy of the reactants and products?

ΔHrxn = Hproducts - Hreactants