The creation of liquid methanol is accomplished by the hydrogenation of carbon monoxide: CO (g) + 2 H 2 (g) → CH 3 OH (l) ∆Hº = – 128.1 kJ How much heat (in kJ) is released when 125.0 g CO reacts with 2.32 x 10 2 g H 2 ?

Here it says the creation of liquid methanol was accomplished by the hydrogenation of carbon monoxide. Here, the delta h associated with the reaction is given as negative 128 point 1 kilojoules. Here they're asking me to determine how much heat in kilojoules is released. So that's us having to find the delta h of unknown. When 125 grams of carbon monoxide, so this is a grams of given grams of given reacts with 2.32 times 10 to the 2 grams of h 2. So here we have a second grams of given. Now remember, if we have more than one given amount that means that this is a limiting reagent type of question. So here we're gonna start out with 125 grams of carbon monoxide. We're gonna change those grams of given into moles of given. So the weight of carbon monoxide is 1 carbon and 1 oxygen, which together comes out to 28.01 grams. Then we're gonna say according to my balanced equation for every one mole of carbon monoxide, we have our delta h as negative 128.1 kilojoule. This comes out as negative 571.67 kilojoules. Now we do the same thing with the h 2. So here we're gonna change the grams of given again into moles of given. So one mole of h 2 weighs 2.016 grams for the 2 hydrogens. And according to our balance equation, for every 2 moles of h 2 we have the same h, delta h of reaction, which is negative 128.1 kilojoule. Here this gives us negative 7 370.833 kilojoules. Now remember, if we're dealing with limiting reagent, we always choose a smaller answer. That represents our theoretical yield. So this would be our answer here, and if we wanna do it in terms of 3 sig figs because of the 2.32, it comes out to negative 572 kilojoules for the amount of heat that's released within our reaction when both of these compounds react with one another.

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7. Energy, Rate and Equilibrium

Thermochemical Equations

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Multiple Choice

The creation of liquid methanol is accomplished by the hydrogenation of carbon monoxide:
CO (g) + 2 H₂ (g) → CH₃OH (l) ∆Hº = – 128.1 kJ
How much heat (in kJ) is released when 125.0 g CO reacts with 2.32 x 10² g H₂?

275 kJ

-572 kJ

-128 kJ

281 kJ

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Verified step by step guidance

First, determine the molar mass of carbon monoxide (CO) and hydrogen (H2). The molar mass of CO is approximately 28.01 g/mol, and the molar mass of H2 is approximately 2.02 g/mol.

Calculate the number of moles of CO and H2 using their respective masses. For CO, use the formula: moles of CO = mass of CO / molar mass of CO. For H2, use: moles of H2 = mass of H2 / molar mass of H2.

Identify the limiting reactant by comparing the mole ratio from the balanced chemical equation to the calculated moles. The balanced equation shows that 1 mole of CO reacts with 2 moles of H2.

Use the limiting reactant to determine the amount of heat released. Since the reaction releases 128.1 kJ per mole of CO reacted, multiply the moles of the limiting reactant by the enthalpy change (∆Hº = -128.1 kJ/mol) to find the total heat released.

Ensure the sign of the heat change is negative, indicating that the reaction is exothermic and releases heat. This will give you the total heat released in kJ.