Question

How many kilograms of C3H6 are needed along with an excess of ammonia to react with
1.31 x 10³ g of O₂ in the following reaction? Use the drop down menus in each section of
the grid to select the best quantity to go in that section of the grid. Use the drop down
menu in the answer box to select the best answer.
2 C3H6(g) + 2 NH3(g) + 3 O₂(g) → 2 C3H3N(g) + 6 H₂O(g)

Answer 1

1.15 kg of  C₃H₆ is needed for the reaction.

What is Moles ?

Mole is a unit of measurement that is equal to the molar mass os an element.

It is given that in the reaction

2 C₃H₆(g) + 2 NH₃(g) + 3 O₂(g) → 2 C₃H₃N(g) + 6 H₂O(g)

Ammonia is present in excess

Oxygen = 1.31 x 10³ g

Propane = ?

Oxygen present in moles = 1.31 x 10³ / 32 = 40.94 moles

The mole ratio of O₂ : C₃H₆ = 3 : 2

Let x be the moles required of C₃H₆

Therefore

40.94 / x = 3 / 2

x = 27.29

Molar mass of C₃H₆ = 42 gm

The amount of C₃H₆ required = 42 * 27.29 = 1146.18 g

The amount of C₃H₆ required = 1.15 kg

Therefore 1.15 kg of  C₃H₆ is needed for the reaction.

To know more about Moles

https://brainly.com/question/26416088

#SPJ1