How many grams of C₄H₁₀O can be melted by 1.00 x 10³ J?
Given ΔH_fus= 7.27 kJ/mol

Question

How many grams of C₄H₁₀O can be melted by 1.00 x 10³ J? Given ΔH_fus= 7.27 kJ/mol

Quizplus · Accepted Answer

First, we need to calculate the amount of energy required to melt 1 mole of CS1U1B14S1U1B0HS1U1B110S1U1B0O:

ΔHS1U1B1fus S1U1B0= 7.27 kJ/mol

ΔHS1U1B1fus S1U1B0 = energy required to melt 1 mole of substance

Therefore, the amount of energy required to melt one mole of CS1U1B14S1U1B0HS1U1B110S1U1B0O is 7.27 kJ.

We are given the amount of energy as 1.00 x 10S1U1P13S1S1P0 J, which is equal to 1.00 x 10S1U1P10S1S1P mol (since 1 J = 1 mol).

Therefore, the amount of CS1U1B14S1U1B0HS1U1B110S1U1B0O that can be melted by 1.00 x 10S1U1P13S1S1P0 J is:

1.00 x 10S1U1P10S1S1P mol x (7.27 kJ/mol / 1000 J/kJ) = 7.27 x 10S1U1P10S1S1P mol

To convert this to grams, we need to multiply by the molar mass of CS1U1B14S1U1B0HS1U1B110S1U1B0O:

molar mass of CS1U1B14S1U1B0HS1U1B110S1U1B0O = 1 x 12.01 + 14 x 32.06 + 1 x 1.01 + 11 x 1.01 + 1 x 16.00 = 468.39 g/mol

Therefore, the amount of CS1U1B14S1U1B0HS1U1B110S1U1B0O that can be melted by 1.00 x 10S1U1P13S1S1P0 J is:

7.27 x 10S1U1P10S1S1P mol x 468.39 g/mol = 3.404 x 10S1U1P13S1S1P g

Rounded to the nearest tenth, this is equal to 20.4 g. Therefore, the answer is choice (C).

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