# Chemistry

At 1 atm, how much energy is required to heat 35.0 g of H2O(s) at –12.0 °C to H2O(g) at 127.0 °C?

1. 👍
2. 👎
3. 👁
1. Do this in steps and add each step to find total q.
1. Within a phase the formula is
q = mass x specfic heat x (Tfinal-Tinitial).
For example to heat 20g liquid water at zero C to 100 C (all in the same phase)
q = 20 x specific heat x (100-0) = ?

2. At the phase change (solid to liquid or liquid to vapor) it is
q = mass x heat fusion at freezing point or
q = mass x heat vaporization at the boiling point.
Then add the q values together to find the total.

1. 👍
2. 👎

## Similar Questions

1. ### Science

1. How much heat energy is lost by 3 kg of water when it cools from 80 degrees C to 10 degrees C? 2. A 300 g piece of aluminum is heated from 30 degrees C to 150 degrees C. What amount of heat energy is absorbed? 3. Determine the

2. ### Science

"Most of the solar radiation is absorbed by the atmosphere and much of what reaches the earth's surface is radiated back into the atmosphere to become heat energy." What can you conclude about heat energy? Most of the sun's energy

3. ### Chemistry

CH4 + 2 O2 --> CO2 + 2 H2O + heat This reaction is exothermic because more energy is released when the products bond than is required to break the bonds of the reactants. The potential energy of the products (not including the

4. ### chemistry

The specific heat of iron is approximately 0.45 J/g °C. How much heat energy is required to raise a 40 g sample of aluminum from 40 °C to 60 °C?

1. ### physics

calculate the amount of heat energy required to melt a 1kg iron ingot initially at 20 ¡ãC? (heat of fusion for Fe is 33.0 J/g

2. ### Chemistry

Two 20.0-g ice cubes at –20.0 °C are placed into 295 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts. Heat capacity of

3. ### Chemistry

which of the following quantities is not required to calculate the amount of heat energy required to heat water from 25^OC to 55^OC? A-the mass of water sample. B-the initial temp. C-the heat of vaporization for water. D-the final

4. ### AP chemistry

The specified heat capacity of silver is 0.24 J/C.g. Please help with this Ap chem quastion.? a. Calculate the energy required to raise the temperature of 150.0 g Ag from 273 K to 298. b. Calculate the energy required to raise the

1. ### Chemistry-Dr.Bob, I need you!!!!

You can mix 100.mL of 1.0 M HCl with 100 mL of 1.0 NaOH, both at 25 degree Celcius. The temperature of your calorimeter rises by 5.98 degree C, and its heat capacity is 100 J/degre C. How much energy is released per mol of H2O

2. ### chemistry

Thermochemistry: 1. Calculate the amount of heat required to decompose 3.5 moles of sodium bicarbonate. 2NaHCO3 + 129 kJ  Na2CO3 + H2O + CO2 In this question, the heat of the reaction is part of the question instead of being

3. ### Chemistry

I have this problem: How much heat energy is required to raise the temperature of 0.365kg of copper from 23.0 ∘C to 60.0 ∘C? The specific heat of copper is 0.0920 cal/(g⋅∘C). I did the equation using formula Heat= mass x

4. ### chem

The specific heat capacity of silver is 0.24 J/°C·g. (a) Calculate the energy required to raise the temperature of 140.0 g Ag from 273 K to 295 K. J (b) Calculate the energy required to raise the temperature of 1.0 mol Ag by