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Numerical Response (1 mark) 1. The minimum amount of heat energy required to completely evaporate 150 g of water expressed in scientific notation , is btimes 10^ast J. If the heat of fusion of water is 6.01kJ/mol and water's heat of vaporization is 40.65kJ/mol, what is the value of b correct to three significant digits? (Record your answer in the box on the right).

Question

Numerical Response (1 mark) 1. The minimum amount of heat energy required to completely evaporate 150 g of water expressed in scientific notation , is btimes 10^ast J. If the heat of fusion of water is 6.01kJ/mol and water's heat of vaporization is 40.65kJ/mol, what is the value of b correct to three significant digits? (Record your answer in the box on the right).

Numerical Response (1 mark)
1. The minimum amount of heat energy required to completely evaporate
150 g of water expressed in scientific notation , is btimes 10^ast J. If the heat
of fusion of water is 6.01kJ/mol and water's heat of vaporization is
40.65kJ/mol, what is the value of b correct to three significant digits?
(Record your answer in the box on the right).

Solution

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SilasExpert · Tutor for 3 years

Answer

Here's how to solve this problem:<br /><br />1. **Calculate the moles of water:**<br /> * The molar mass of water (H₂O) is approximately 18.015 g/mol.<br /> * Moles of water = mass / molar mass = 150 g / 18.015 g/mol ≈ 8.326 mol<br /><br />2. **Calculate the energy required for vaporization:**<br /> * Energy = moles × heat of vaporization <br /> * Energy = 8.326 mol × 40.65 kJ/mol = 338.3 kJ<br /><br />3. **Convert to joules and scientific notation:**<br /> * Energy = 338.3 kJ × 1000 J/kJ = 338300 J<br /> * In scientific notation, this is 3.383 × 10⁵ J<br /><br />4. **Identify the value of b:**<br /> * The question asks for the value of *b* in the expression *b* × 10^* J.<br /> * Therefore, *b* = 3.38 (rounded to three significant figures).<br /><br />**Final Answer:** 3.38<br />
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