The value of ƒ¢H�‹ 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)
*I just want to how to solve this problem as in an equation, not the answer. thank you!
I thought I did this for you a day or so ago.
482*(12.0/2*molar mass CO) = ?
To calculate the heat released to the surroundings when 12.0 g of CO(g) reacts completely, you can use the following steps:
1. First, convert the mass of CO(g) to moles. To do this, divide the given mass (12.0 g) by the molar mass of CO, which you can find from the periodic table.
2. Next, balance the given reaction equation so that the moles of CO and CO2 are proportional. In this case, it appears that the reaction is already balanced, with a 2:2:1 ratio.
3. Use the balanced equation to determine the moles of CO2 produced. Since the stoichiometry of the reaction tells us that 2 moles of CO produce 2 moles of CO2, you can use the mole ratio to calculate the moles of CO2 formed.
4. Finally, utilize the given value of ∆H for the reaction (-482 kJ) along with the moles of CO2 produced to calculate the heat released to the surroundings. The heat released can be determined by multiplying the moles of CO2 by the value of ∆H.
Make sure to follow each step accurately and double-check your calculations to ensure the accuracy of your final answer.