How many grams of water could have its temperature raised from 25 ºC (room temperature) to 100 ºC (the boiling point of water) by the amount of energy released in the formation of 4.0 mol of H2 from hydrogen atoms? The bond energy of H2 is 435 kJ/mol. The specific heat of water is 4.184 J/g °C. Express your answer in scientific notation.
q = 4 mol x 435 kJ/mol = ? kJ = ? x 1000 J.
q = mass x specific heat x (Tfinal-Tinitial). YOu know Tfinal, Tinitial, specific heat, and q, solve for mass
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To solve this problem, we need to follow a series of steps:
Step 1: Calculate the energy released in the formation of 4.0 mol of H2 from hydrogen atoms.
The bond energy of H2 is given as 435 kJ/mol. Therefore, the energy released can be calculated as follows:
Energy released = Bond energy × Number of moles
Energy released = 435 kJ/mol × 4.0 mol
Let's calculate this energy:
Energy released = 1740 kJ
Step 2: Calculate the amount of heat required to raise the temperature of water.
The specific heat of water is given as 4.184 J/g °C. This means that it takes 4.184 Joules of energy to raise the temperature of 1 gram of water by 1 °C.
Step 3: Calculate the mass of water that can be heated.
We need to determine the mass of water that can have its temperature raised by the energy released during the formation of H2. Let's assume that all the energy released is used to heat the water.
Now, we can use the formula:
Energy = mass × specific heat × temperature change
Rearranging the formula to solve for mass:
Mass = Energy / (specific heat × temperature change)
In this case, the temperature change is:
Temperature change = Final temperature - Initial temperature
Temperature change = 100 °C - 25 °C
Temperature change = 75 °C
Plugging in the values:
Mass = 1740 kJ / (4.184 J/g °C × 75 °C)
Let's calculate the mass now:
Mass = 5.869 grams
Thus, you can raise the temperature of approximately 5.869 grams of water from 25 ºC to 100 ºC using the energy released in the formation of 4.0 mol of H2 from hydrogen atoms.