Thermochemistry Intro

How many grams of Aluminum are needed to raise the temperature by 12°C, and using 50 J of energy? Specific heat of Aluminum is 0.902 J/g•°C

• 4.62 grams

• 4.58 grams

• 4.92 grams

• 5.01 grams

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-2

NGSS.HS-PS3-4

How much heat is produced when 57 grams of Lead is heated from 45°C to 67°C. The specific heat of Lead is 0.128 J/g•°C.

• 8.289 Joules

• 185,142 Joules

• 185.142 Joules

• 160.512 Joules

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

The amount of heat that raises the temperature of 1 g of pure water 1°C

• energy

• calorie

• heat capacity

• exothermic process

Tags

NGSS.HS-PS3-4

The capacity to do work or to supply heat

• heat capacity

• specific heat

• enthalpy

• energy

Tags

NGSS.HS-PS3-4

What type of reaction is this?

• Exothermic

• Endothermic

• Kinetic

• Potential

Tags

NGSS.HS-PS1-4

H₂ + ½ O₂ --> H₂O + 285kJ is an example of a(n)

• Electrical equation

• Heat equation

• Thermochemical equation

Tags

NGSS.HS-PS1-4

Twenty tortilla chips are combusted in a bomb calorimeter surrounded by 5 liters of water. The temperature of the water increases from 30℃ to 35℃. Assuming the heat capacity of the water is about 4 J/g∙ ℃ and the heat capacity of the calorimeter 2000 J/℃, what is the energy content of a single tortilla chip?

• 100 kJ

• 110 kJ

• 5.5 kJ

• 5 kJ

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

A 50 gram sample of delicious pork rinds is placed in an open, constant pressure calorimeter that contains 3000 grams of water. The temperature of the water increases by 47℃ when the pork rinds are combusted. The heat capacity for water is 4.184 J/g ∙ ℃. Assume the heat lost to the calorimeter itself or to the air is negligible. Which of the following is correct for the SYSTEM?

• ∆H = -590 kJ

• ∆H = +590 kJ

• ∆H = -11.8 kJ

• ∆H = +11.8 kJ

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

A positive ΔH means that:

• In order for the reaction to happen, heat must be input. It is exothermic

• In order for the reaction to happen, heat must be input. It is endothermic.

• When the reaction happens, heat is released. It is exothermic

• When the reaction happens, heat is released. It is endothermic

Tags

NGSS.HS-PS1-4

What is true about thermodynamically favorable reactions?

• They need outside energy to be put in

• They always increase entropy

• They always have a negative ΔH

• ΔG is positive