Question

Consider this reaction.

2N2H4(l) + N2O4(l) -> 3N2(g) + 4H2O (g)
H=-1078 kJ
How much energy is released by this reaction during the formation of 140. g of N2(g) ?

Answer 1

The energy released by the reaction can be found by multiplying the moles of N2 by the enthalpy change. In this case, the energy released is -5390 kJ.

Step-by-step explanation:

The energy released by the reaction can be determined using the equation q = mcΔT, where q is the energy released, m is the mass of the substance, c is the specific heat capacity, and ΔT is the change in temperature. In this case, we are given the enthalpy change (H) for the reaction, which is -1078 kJ. We are also given the molar mass of N2, which is 28 g/mol. To find the energy released during the formation of 140 g of N2, we need to calculate the moles of N2, which is given by moles = mass / molar mass. Then, we can use the equation q = moles * enthalpy change to find the energy released.

First, calculate the moles of N2: moles = 140 g / 28 g/mol = 5 moles

Next, calculate the energy released: q = 5 moles * (-1078 kJ/ 1 mole) = -5390 kJ

Therefore, the energy released during the formation of 140 g of N2 is -5390 kJ.