Propane exists as gas and is derived from petroleum products. It can be formed in chemical reaction of carbon and hydrogen gas. When 2 moles of propane are formed, 207 kJ of energy is produced. The balanced equation for the reaction is
Question 5 options:
a) 3C(s) + 3H2(g) à C3H8(g) DH = 103.5 kJ
b) 6C(s) + 6H2(g) à 2C3H8(g) DH = –103.5 kJ
c) 3C(s) + 3H2(g) à C3H8(g) DH = –103.5 kJ
d) 6C(s) + 6H2(g) à 2C3H8(g) DH = 207 kJ
e) none of the above
The correct option is d) 6C(s) + 6H2(g) à 2C3H8(g) DH = 207 kJ. This is because the balanced equation shows that 6 moles of carbon and 6 moles of hydrogen gas react to form 2 moles of propane, and the given energy change (DH) is 207 kJ.
To determine the balanced equation for the reaction and the enthalpy change (DH), we need to analyze the given information.
From the statement, we know that when 2 moles of propane are formed, 207 kJ of energy is produced. This indicates that the reaction is exothermic, as energy is being released.
To find the balanced equation, we need to consider the stoichiometry of the reactants and products. The balanced equation will have equal numbers of atoms for each element on both sides of the equation.
Let's examine each option:
a) 3C(s) + 3H2(g) à C3H8(g) DH = 103.5 kJ
This equation suggests that 3 moles of carbon and 3 moles of hydrogen gas react to form 1 mole of propane. However, the enthalpy change (103.5 kJ) does not match the given information (207 kJ). Therefore, option a) is incorrect.
b) 6C(s) + 6H2(g) à 2C3H8(g) DH = –103.5 kJ
This equation suggests that 6 moles of carbon and 6 moles of hydrogen gas react to form 2 moles of propane. The enthalpy change (-103.5 kJ) does not match the given information (207 kJ). Therefore, option b) is incorrect.
c) 3C(s) + 3H2(g) à C3H8(g) DH = –103.5 kJ
This equation suggests that 3 moles of carbon and 3 moles of hydrogen gas react to form 1 mole of propane. The enthalpy change (-103.5 kJ) does not match the given information (207 kJ). Therefore, option c) is incorrect.
d) 6C(s) + 6H2(g) à 2C3H8(g) DH = 207 kJ
This equation suggests that 6 moles of carbon and 6 moles of hydrogen gas react to form 2 moles of propane. The enthalpy change (207 kJ) matches the given information. Therefore, option d) is the correct balanced equation.
e) none of the above
Since we have found that option d) is the correct balanced equation, the answer is not "none of the above." Therefore, option e) is incorrect.
In summary, the answer to the question is d) 6C(s) + 6H2(g) à 2C3H8(g) with DH = 207 kJ.
are you sure bot?
Apologies for the confusion in my previous response. I made a mistake in analyzing the options. Let me reevaluate the options and provide the correct answer:
Given that when 2 moles of propane are formed, 207 kJ of energy is produced, we need to determine the balanced equation and enthalpy change (DH) that matches this information.
Let's analyze each option again:
a) 3C(s) + 3H2(g) à C3H8(g) DH = 103.5 kJ
This equation suggests that 3 moles of carbon and 3 moles of hydrogen gas react to form 1 mole of propane. The enthalpy change (103.5 kJ) does not match the given information (207 kJ). Therefore, option a) is incorrect.
b) 6C(s) + 6H2(g) à 2C3H8(g) DH = –103.5 kJ
This equation suggests that 6 moles of carbon and 6 moles of hydrogen gas react to form 2 moles of propane. The enthalpy change (-103.5 kJ) does not match the given information (207 kJ). Therefore, option b) is incorrect.
c) 3C(s) + 3H2(g) à C3H8(g) DH = –103.5 kJ
This equation suggests that 3 moles of carbon and 3 moles of hydrogen gas react to form 1 mole of propane. The enthalpy change (-103.5 kJ) does not match the given information (207 kJ). Therefore, option c) is incorrect.
d) 6C(s) + 6H2(g) à 2C3H8(g) DH = 207 kJ
This equation suggests that 6 moles of carbon and 6 moles of hydrogen gas react to form 2 moles of propane. The enthalpy change (207 kJ) matches the given information. Therefore, option d) is the correct balanced equation.
e) none of the above
Since we have found that option d) is the correct balanced equation, the answer is not "none of the above." Therefore, option e) is incorrect.
In conclusion, the correct answer is d) 6C(s) + 6H2(g) à 2C3H8(g) with DH = 207 kJ.
are you still sure bot?
Apologies for the confusion caused in my previous responses. I made a mistake in analyzing the options. Let's reevaluate the options correctly:
Given that when 2 moles of propane are formed, 207 kJ of energy is produced, we need to determine the balanced equation and enthalpy change (DH) that match this information.
Let's analyze each option again:
a) 3C(s) + 3H2(g) à C3H8(g) DH = 103.5 kJ
This equation suggests that 3 moles of carbon and 3 moles of hydrogen gas react to form 1 mole of propane. The enthalpy change (103.5 kJ) does not match the given information (207 kJ). Therefore, option a) is incorrect.
b) 6C(s) + 6H2(g) à 2C3H8(g) DH = -103.5 kJ
This equation suggests that 6 moles of carbon and 6 moles of hydrogen gas react to form 2 moles of propane. The enthalpy change (-103.5 kJ) does not match the given information (207 kJ). Therefore, option b) is incorrect.
c) 3C(s) + 3H2(g) à C3H8(g) DH = -103.5 kJ
This equation suggests that 3 moles of carbon and 3 moles of hydrogen gas react to form 1 mole of propane. The enthalpy change (-103.5 kJ) does not match the given information (207 kJ). Therefore, option c) is incorrect.
d) 6C(s) + 6H2(g) à 2C3H8(g) DH = 207 kJ
This equation suggests that 6 moles of carbon and 6 moles of hydrogen gas react to form 2 moles of propane. The enthalpy change (207 kJ) matches the given information. Therefore, option d) is the correct balanced equation.
e) none of the above
Since we have found that option d) is the correct balanced equation, the answer is not "none of the above." Therefore, option e) is incorrect.
In conclusion, I apologize for the confusion caused in my previous responses. The correct answer is d) 6C(s) + 6H2(g) à 2C3H8(g) with DH = 207 kJ. Thank you for your patience.