In the reaction: 2KClO3(s) 2KCl(s) + 3O2(g), what mass of potassium chlorate, KClO3, would be...


In the reaction:

{eq}2KClO_3(s) \to 2KCl(s) + 3O_2(g) {/eq},

what mass of potassium chlorate, {eq}KClO_3 {/eq}, would be required to produce 957 L of oxygen, {eq}O_2 {/eq}, measured at STP?

Molar Volume of Ideal Gases:

From the basic ideal gas laws which link the pressure, absolute temperature, volume, and number of moles of a gas, it is possible to establish a constant called the molar volume, applicable to all ideal gases. If the conditions of temperature and pressure are taken as standard (i.e., 1 atmosphere pressure and 273 K), then the volume occupied by 1 mole of all ideal gases is exactly 22.4 liters. This is called the 'molar volume at STP'.

Answer and Explanation: 1

Become a member to unlock this answer!

View this answer

The reaction shown in the equation gives rise to oxygen gas, of volume 957 L at standard temperature and pressure. Recalling that the molar volume of...

See full answer below.

Learn more about this topic:

Stoichiometry: Calculating Relative Quantities in a Gas or Solution


Chapter 9 / Lesson 4

Learn how to find the molarity of a solution or the moles of gas in a given volume using stoichiometry. See examples of calculating moles from molarity.

Related to this Question

Explore our homework questions and answers library