Question

A 1.80-gram mixture of potassium chlorate and potassium chloride is heated until all of the potassium chlorate has decomposed. after being dried, the liberated oxygen occupies a volume of 405 ml at 25oc and 745 torr. how many moles of oxygen were produced?

Answer 1

The question involves using the ideal gas law to calculate the number of moles of oxygen produced from the decomposition of potassium chlorate, a common high school level chemistry problem.

Step-by-step explanation:

The subject of this question is Chemistry, and it pertains to a high school level of education. Determining how many moles of oxygen were produced involves using the ideal gas law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

To find the number of moles of oxygen gas produced, you first need to convert the temperature to Kelvin (25°C + 273.15 = 298.15 K) and the pressure to atmospheres (1 atm = 760 torr, so 745 torr = 745/760 atm). Using the given volume (405 ml or 0.405 L), you can then solve for n (moles of oxygen) using the ideal gas law equation with R = 0.0821 L·atm/K·mol.

Here's the calculation:

(745 torr / 760 torr/atm) × 0.405 L = n × 0.0821 L·atm/K·mol × 298.15 K

Solving for n, you can determine the number of moles of oxygen produced.

This exercise typically involves chemistry concepts such as the decomposition of chemical compounds, the collection and measurement of gases, and calculations using the ideal gas law equation.