TIA - Thermochemistry

A reaction that releases heat is— (TEKS 13(A))

• Endothermic

• Exothermic

• Neutral

• Reversible

Answer explanation

Tags

NGSS.HS-PS1-4

What is the specific heat capacity of water? (TEKS 13(B))

• 1.0 cal/g°C

• 4.18 J/g°C

• 2.5 J/g°C

• 0.5 cal/g°C

Answer explanation

The answer to this is in your REFERENCE MATERIAL and also in other questions in this topic.

Tags

NGSS.HS-PS3-4

In an endothermic reaction, the enthalpy change (ΔH) is— (TEKS 13(C))

• Positive

• Negative

• Zero

• Undefined

Answer explanation

Tags

NGSS.HS-PS1-4

Breaking bonds in a reaction requires— (TEKS 13(D))

• Energy release

• Energy absorption

• No energy change

• Temperature decrease

Answer explanation

Tags

NGSS.HS-PS1-4

What measures the heat of a reaction at constant pressure? (TEKS 13(C))

• Entropy

• Enthalpy

• Kinetic energy

• Activation energy

Answer explanation

A reaction has ΔH = -50 kJ/mol and feels warm. What type is it? (TEKS 13(A))

• Endothermic

• Exothermic

• Isothermic

• Adiabatic

Answer explanation

Tags

NGSS.HS-PS1-4

How much heat raises 100 g of water from 25°C to 75°C? (c = 4.18 J/g°C) (TEKS 13(B))

• 1045 J

• 2090 J

• 20,900 J

• 41,800 J

Answer explanation

Tags

NGSS.HS-PS3-1

If reactants have 200 kJ of energy and products have 150 kJ, what is ΔH, and is heat released or absorbed? (TEKS 13(C))

• -50 kJ, released

• +50 kJ, absorbed

• -50 kJ, absorbed

• +50 kJ, released

Answer explanation

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1

Why is bond formation exothermic? (TEKS 13(D))

• Energy is absorbed to stabilize the bond

• Energy is released to stabilize the bond

• Energy is absorbed to break the bond

• Energy is released to break the bond

Answer explanation

Tags

NGSS.HS-PS1-4

A reaction requires 75 kJ to break bonds and releases 100 kJ when forming bonds. What is ΔH? (TEKS 13(C))

• -25 kJ

• +25 kJ

• -175 kJ

• +175 kJ

Answer explanation

Tags

NGSS.HS-PS1-4