An exothermic reaction releases 13,450J of heat. How many calories of energy are released? A) 5 56,274 calories B)1,244 caloriesC) 134,500 caloriesD) 3,215 calories

The correct option is;

D) 3,215 calories

Explanation:

Here we are required to convert 13,450 J to calories

1 calorie is the amount of heat required to raise the temperature of 1 gram of water by 1°C

Therefore, 1 calorie = 4.184 Joules

Hence, 1 Joule = 1/4.184 calorie for which we have;

13,450 J = 13,450 × 1/4.184 calories = 13,450/4.184 calorie

13,450 J = 3,214.63 calories

Rounding up to the nearest  whole number, we have;

13,450 J ≈ 3,215 calories.

n2(g) + 3h2-> 2nh3(g)   this is the balanced equation

note the mole ratio between n2, h2 and nh3.   it is 1 : 3 : 2   this will be important.

moles n2 present = 28.0 g n2 x 1 mole n2/28 g = 1 mole n2 present

moles h2 present = 25.0 g h2 x 1 mole h2/2 g = 12.5 moles h2 present

based on mole ratio, n2 is limiting in this situation because there is more than enough h2 but not enough n2.

moles nh3 that can be produced = 1 mole n2 x 2 moles nh3/mole n2 = 2 moles nh3 can be produced

grams of nh3 that can be produced = 2 moles nh3 x 17 g/mole = 34 grams of nh3 can be produced

note:   the key to this problem is recognizing that n2 is limiting, and therefore limits how much nh3 can be produced.

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