Question

Liquid methanol (CH₃OH) can be used as an alternative fuel in pickup and SUV engines. An industrial method for preparing it involves the catalytic hydrogenation of carbon monoxide:
CO(g) + 2H₂(g) → CH₃OH(l)
How much heat (in kJ) is released when 15.0 L of CO at 85°C and 112 kPa reacts with 18.5 L of H₂ at 75°C and 744 torr?

Answer 1

40.6 kJ of heat energy had been emitted.

CO(g) + 2H2(g) CH3OH(l)CO volume, V (CO), equals 15 L or 0.015 m3.

Temperature = 85 0C = 85 + 273 = 358 K Pressure = 112 kPa = 112,000 PaPV = nRT n= 112000 0.015 / 8.314 358 n(CO) = 0.56 moles,

according to the ideal gas law.H2 volume is 14.4 L or 0.0144 m3

T = 750C + 273 K = 348 K n(H2) = 99191.84 0.0144 m3 / 8.314 348 K = 0.49 moles of H2 Pressure = 744 torr = 99191.84 Pa

Hydrogen is the limiting reagent, according to the calculation above.CH3OH = H2 = 0.49/2 = 0.245 m-238.6 (-110.5) = -128.1 kJ/mol for H(rxn) = H(f) (CH3OH) - H (rxn)

We must now multiply H(rxn) by the number of moles of methanol.

E = H(rxn) n(CH3OH) = 128.1 0.245 = 40.6 kJ.

Learn more about Ideal gas law here-

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