Question

question 3 (1 point)
how much heat is 1 evolved/absorbed when 2.22 x 10² moles of n₂ are consumed? (answer = 9.77 x 10³ kj)
n₂ + 3 br₂ → 2 nbr₃ + 44.0 kj
this reaction is 2 endothermic/exothermic
3 kj
(2.22 x 10² mol n₂)(----------) = 4 kj
5 mol n₂
a. 1 b. 2 c. 3 d. 4 e. 5 f. 253.719 g. 3.38 x 10⁰
h. 3.26 x 10³ i. 44.0 j. 1.33 x 10⁻² k. 9.77 x 10³ l. 4.44 x 10²
m. 6.66 x 10² n. 500.0 o. 556 p. 90.0 q. 3.2852 r. 159.81
s. 28.013 t. 1.750 u. 0.8750 v. 13.0 w. 0.46306 x. 1.3892
y. 24.5 z. 38.5 aa. 2.190 bb. evolved cc. absorbed
dd. exothermic ee. endothermic

Explanation:

Step1: Determine heat evolution/absorption

Since heat (\(44.0\ kJ\)) is on the product side of the reaction \(N_{2}+3Br_{2}\to2NBr_{3}+44.0\ kJ\), heat is evolved.

Step2: Determine reaction type

Reactions that evolve heat are exothermic.

Step3: Set up mole - heat conversion

From the balanced equation, \(1\ mol\ N_{2}\) corresponds to \(44.0\ kJ\) of heat evolved.

Step4: Calculate heat for \(2.22\times10^{2}\ mol\ N_{2}\)

\((2.22\times 10^{2}\ mol\ N_{2})\times\frac{44.0\ kJ}{1\ mol\ N_{2}}=(2.22\times44.0)\times10^{2}\ kJ = 9.77\times 10^{3}\ kJ\)

Answer:

1. BB. evolved
2. DD. exothermic
3. I. \(44.0\)
4. K. \(9.77\times 10^{3}\)
5. A. \(1\)