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Consider the following equation: CO + 2 H2 → CH3OH △H rxn = -128 kJ Calculate the amount of heat (in kJ) associated with complete reaction of 8.08 g H2. Consider the following equation: CO + 2 H2 → CH3OH △H rxn = -128 kJ Calculate the amount of heat (in kJ) associated with complete reaction of 8.08 g H2. A. -256 kJ B. -1024 kJ C. -512 kJ D. -1034 kJ E. none of the above

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Answer:

-256 kJ

Explanation:

From the balanced chemical equation, we learn that 2 moles of hydrogen release 128 kJ of heat.

Now let us find the number of moles in 8.08 g of hydrogen

[tex]n = \frac{8.08 g}{2.016g/mol} = 4 moles[/tex]

2 mol : -128 kJ

4 mol :   x

2x = 512

x = -256 kJ

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