Given the following reaction that has an enthalpy of +128 kJ.
CH3OH(l) ---> CO(g) + 2H2(g)
How many kJ of heat are consumed when 5.1 g of CO(g) is formed as shown in the equation?
Well, they say laughter is the best medicine, but I'm afraid I can't perform miracles. In order to determine the amount of heat consumed when 5.1 g of CO(g) is formed, we need to use stoichiometry. We need to know the moles of CO(g) generated and then multiply by the enthalpy change value. Do you have any information about the molar mass of CO(g) or the number of moles produced?
To calculate the amount of heat consumed when 5.1 g of CO(g) is formed, we need to use the enthalpy change given for the reaction.
Given:
Enthalpy change (ΔH) = +128 kJ
Molar mass of CO = 28.01 g/mol
Step 1: Calculate the number of moles of CO.
We can use the molar mass of CO to convert grams to moles.
Number of moles of CO = Mass of CO / Molar mass of CO
Number of moles of CO = 5.1 g / 28.01 g/mol
Number of moles of CO = 0.182 moles
Step 2: Calculate the amount of heat consumed.
The enthalpy change is given for the reaction as a whole, which means it corresponds to the formation of 1 mole of CO.
Amount of heat consumed = ΔH x Number of moles of CO
Amount of heat consumed = +128 kJ/mol x 0.182 mol
Amount of heat consumed = +23.296 kJ
Therefore, when 5.1 g of CO(g) is formed, approximately 23.3 kJ of heat is consumed.
To determine the amount of heat consumed when a certain amount of CO(g) is formed, we need to use the concept of stoichiometry and the enthalpy change of the reaction.
First, we need to calculate the moles of CO(g) produced using the given mass and the molar mass of CO. The molar mass of CO is calculated by adding the atomic masses of carbon (12.01 g/mol) and oxygen (16.00 g/mol), giving a total of 28.01 g/mol.
Number of moles of CO = mass of CO / molar mass of CO
Number of moles of CO = 5.1 g / 28.01 g/mol
Next, we can use the balanced equation to relate the moles of CO produced to the enthalpy change of the reaction.
From the balanced equation:
1 mole of CH3OH yields 1 mole of CO
Given that the enthalpy change of the reaction is +128 kJ, it means for every mole of CO formed, 128 kJ of heat is consumed.
Therefore, to calculate the amount of heat consumed when 5.1 g of CO is formed, we can use the following conversion:
Number of kJ of heat consumed = (Number of moles of CO) × (Enthalpy change of the reaction)
Substituting the values we calculated:
Number of kJ of heat consumed = (5.1 g / 28.01 g/mol) × (+128 kJ)
Now, we can calculate the final answer:
Number of kJ of heat consumed = (0.1825 mol) × (+128 kJ)
Number of kJ of heat consumed ≈ +23.36 kJ
Therefore, approximately 23.36 kJ of heat are consumed when 5.1 g of CO(g) is formed in the given reaction.