The dH for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 12.0 g of CO (g) reacts completely.
2CO(g) + O2(g) --> 2CO2(g)
idk
To calculate the heat released to the surroundings, we need to use the following equation:
q = (DH / n) * m
Where:
q is the heat released to the surroundings (in kJ)
DH is the enthalpy change (-482 kJ)
n is the mole ratio of CO in the balanced equation (2 moles of CO)
m is the mass of CO used (12.0 g)
Step 1: Calculate the number of moles of CO used
To calculate the number of moles, we will use the molar mass of CO.
Molar mass of CO = atomic mass of C + atomic mass of O
= (12.01 g/mol) + (16.00 g/mol)
= 28.01 g/mol
Number of moles of CO = mass of CO / molar mass of CO
= 12.0 g / 28.01 g/mol
≈ 0.428 mol
Step 2: Calculate the amount of heat released to the surroundings
Using the equation mentioned above:
q = (DH / n) * m
= (-482 kJ / 2 mol) * 0.428 mol
= -205.88 kJ
Therefore, the heat released to the surroundings when 12.0 g of CO reacts completely is approximately -205.88 kJ. The negative sign indicates that the reaction is exothermic, meaning heat is released.