A 10.0 L vessel contains 0.0015 moles carbon dioxide and 0.10 moles of carbon monoxide. A 5.00 gram sample of carbon is added and the temperature is increased to 1000. degrees C. Will more carbon monoxide form? Kc at 1000 degrees C is 1.17.
CO2(g) + C(s) ⇌ 2CO (g)
To determine if more carbon monoxide (CO) will form when a 5.00 g sample of carbon is added and the temperature is increased to 1000 degrees C, we need to calculate the reaction quotient Qc and compare it to the equilibrium constant Kc.
1. Calculate the number of moles of carbon (C) in the 5.00 g sample.
- First, we need to determine the molar mass of carbon, which is approximately 12.01 g/mol.
- Divide 5.00 g by the molar mass of carbon to find the number of moles of carbon.
2. Determine the initial number of moles of carbon dioxide (CO2) and carbon monoxide (CO) in the 10.0 L vessel.
- Given that the vessel contains 0.0015 moles of CO2 and 0.10 moles of CO.
3. Calculate the initial concentration of CO2 and CO in the vessel.
- Divide the number of moles by the volume of the vessel (10.0 L) to obtain the concentration in moles per liter.
4. Calculate the initial value of Qc.
- Use the formula: Qc = [CO]^2 / [CO2], where [CO] and [CO2] represent the initial concentrations of carbon monoxide and carbon dioxide, respectively.
5. Compare Qc to Kc.
- If Qc is smaller than Kc, it means that the reaction is not yet at equilibrium, and more carbon monoxide will form to reach equilibrium.
- If Qc is larger than Kc, it means that the reaction is already at equilibrium, and no further conversion will occur.
By following these steps and performing the calculations, you can determine whether more carbon monoxide will form when the conditions change.
To determine if more carbon monoxide will form when a carbon sample is added and the temperature is increased, we need to compare the initial moles of carbon dioxide (CO2) and carbon monoxide (CO) with the moles of CO and CO2 that would be present at equilibrium.
1. Calculate the initial moles of CO2 and CO:
- CO2: 0.0015 moles
- CO: 0.10 moles
2. The balanced equation for the reaction is: CO2(g) + C(s) ⇌ 2CO(g), which means that 1 mole of CO2 reacts with 1 mole of C to produce 2 moles of CO.
3. Determine the moles of CO and CO2 at equilibrium:
- Let x be the moles of CO2 and CO formed at equilibrium.
- Since 1 mole of CO2 reacts with 1 mole of C to produce 2 moles of CO, the change in the moles of CO2 would be -x, and the change in the moles of CO would be +2x.
- Therefore, the moles of CO2 at equilibrium would be 0.0015 - x, and the moles of CO at equilibrium would be 0.10 + 2x.
4. The expression for the equilibrium constant (Kc) is given as:
Kc = [CO]^2 / [CO2]
Where [CO] represents the concentration of CO and [CO2] represents the concentration of CO2.
5. Substitute the given values into the equilibrium constant expression:
Kc = (0.10 + 2x)^2 / (0.0015 - x)
6. Since the temperature is increased to 1000 degrees C and the value of Kc is provided at this temperature (Kc = 1.17), we can solve for x:
1.17 = (0.10 + 2x)^2 / (0.0015 - x)
7. Solve the equation to find the value of x. This may involve some algebraic manipulation and solving a quadratic equation. The value of x will represent the moles of CO and CO2 formed at equilibrium.
8. After finding the value of x, substitute it back into the expressions for the moles of CO and CO2 at equilibrium to determine their values.
9. Compare the moles of CO and CO2 at equilibrium with the initial moles to determine if more CO has been formed. If the moles of CO at equilibrium is greater than the initial moles, then more CO has formed.
By following these steps, you can determine whether more carbon monoxide will form when the carbon sample is added and the temperature is increased.