Heat Formulas

What is the specific heat capacity of silver metal if 55 grams of the metal absorbs 47.3 joules of heat and the temperature rises 15 degrees Celcius?

• 0.033 J/gC
• 0.057 J/gC
• 39000 J/gC
• .0455 J/gC

)If the temperature of copper starts at 15°C and increases to 100°C, what is the change in temperature (ΔT)?

• 115
• 100
• 85
• 15

How much heat does an aluminum block absorb if 10.00 grams ae heated from 25.0^oC to 50.0^oC? the specific heat of aluminum is .900J/g^oC

• 450
• -450
• 225
• -225

Tags

NGSS.HS-PS3-1

A 20.0 g sample of iron receives 50.J of heat energy. If iron has a specific heat of 0.10 J/g°C, and starts at a temperature of 30°C what is the final temperature of the iron?

• 25

• 5

• 55

• 50

When 1500J of energy is lost from a 120 gram object, the temperature decreased from 45 degrees C to 40 degrees C. What is the specific heat of the object?

• 2.5 J/gC
• 1.5 J
• 12.5 Cal/gC
• 15 J/gC1 

Tags

NGSS.HS-PS3-1

If the enthalpy (ΔH) is negative the reaction is ____.

• Endothermic
• Exothermic
• Neutral

The enthalpy of vaporatization for methanol is 38.3 kJ/mol. How many moles can be boiled with the input of 258 kJ of heat?

• 6.74 mol

• 0.148 mol

• 9881 mol

• 1.68 mol

The enthalpy of fusion for water is 6.07 kJ/mol. How much heat (in J) is required to melt 15 grams of water?

• 91050 J

• 5058 J

• 5.058 J

• 3580 J

The enthalpy of vaporation for water is 2260 J/g. How many kJ of heat are required to boil 117 grams water?

• 14700 kJ

• 264.4 kJ

• 14.7 kJ

• 358 kJ

How much heat is required to raise 10 grams of water from -5°C to 15°C? Use your heating curve for constants.

• 21010 J

• 4072 J

• 836.8 J

• 732.1 J