The mass of oxygen collected from the thermal decomposition of potassium chlorate at a temperature of 297 K and 762 mmHg is 0.16 g
<h3>How to determine the mole of oxygen produced </h3>
We'll begin by obtaining the number of mole of oxygen gas produced from the reaction. This can be obtained by using the ideal gas equation as illustrated below:
- Volume (V) = 0.128 L
- Temperature (T) = 297 K
- Pressure (P) = 762 – 22.4 = 739.6 mmHg
- Gas constant (R) = 62.363 mmHg.L/Kmol
- Number of mole (n) =?
PV = nRT
739.6 × 0.128 = n × 62.363 × 297
Divide both sides by 62.363 × 297
n = (739.6 × 0.128) / (62.363 × 297)
n = 0.0051 mole
Thus, the number of mole of oxygen gas produced is 0.0051 mole
<h3>How to determine the mass of oxygen collected</h3>
Haven obtain the number of mole of oxygen gas produced, we can determine the mass of the oxygen produced as follow:'
- Mole = 0.0051 mole
- Molar mass of oxygen gas = 32 g/mole
- Mass of oxygen =?
Mole = mass / molar mass
0.0051 = mass of oxygen / 32
Cross multiply
Mass of oxygen = 0.0051 × 32
Mass of oxygen = 0.16 g
Thus, we can conclude that the mass of oxygen gas collected is 0.16 g
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Covalent since they are both non metals, a metal and a non metal make an ionic bond
well, the oil will come up on the surface of the water and lay there but introducing air does not do much. hope that helps
First, find out how many grams are in one mole of CO2(the two oxygen atoms means you need to multiply oxygen’s amu by 2,then add whatever carbon’s amu is to that). Then divide 26 grams by that number and that will be your moles. There are only two significant figures, so round your answer correctly.
