Final answer:
The limiting reactant is CH4 and the expected amount of C2H4N2 is 3.016 g (Option E). The expected amount of C2H4N2 in the reaction can be calculated by determining the limiting reactant and using stoichiometry.
Step-by-step explanation:
The reaction is:
CO2 + NH3 + 3CH4 → 2C2H4N2 + 3H2O
To find the amount of C2H4N2, we need to calculate the moles of each reactant, and then determine the limiting reactant.
The limiting reactant is the reactant that is completely consumed and limits the amount of product that can be formed.
First, calculate the moles:
- 14.5 g CO2 x (1 mole CO2 / 44.01 g CO2) = 0.329 mol CO2
- 2.07 g NH3 x (1 mole NH3 / 17.03 g NH3) = 0.121 mol NH3
- 1.81 g CH4 x (1 mole CH4 / 16.04 g CH4) = 0.113 mol CH4
Next, use the stoichiometry of the balanced equation to determine the moles of C2H4N2 that can be expected:
From the balanced equation, 3 moles of CH4 react to form 2 moles of C2H4N2.
Therefore, the moles of C2H4N2 can be calculated as:
0.113 mol CH4 x (2 mol C2H4N2 / 3 mol CH4) = 0.0753 mol C2H4N2
Finally, convert the moles of C2H4N2 to grams:
0.0753 mol C2H4N2 x (40.03 g C2H4N2 / 1 mol C2H4N2) = 3.016 g C2H4N2
Therefore, the expected amount of C2H4N2 is 3.016 g (Option E).
The complete question is:
How much C2H4N2 could be expected from the reaction of 14.5 g CO2, 2.07 g NH3, and 1.81 g CH4?
a) 0.2 g C2H4N2
b) 0.5 g C2H4N2
c) 1.0 g C2H4N2
d) 2.0 g C2H4N2
e) 3.016g C2H4N2