⚛ the first letter of the chemical symbol of an element is always a capital letter (upper case letter) The chemical symbol of an element can be made up of either 1 letter or 2 letters: This chemical symbol of an element is most often based on the current name of the element, or, in some cases, it is based on an older name for the element. ![]() In addition, there are more than 20 man-made elements (synthetic elements or artifical elements).Īll the known elements, both naturally occurring and synthetic elements, are listed in the Periodic Table of the Elements.Įach element has been given a unique name and a unique chemical symbol. There are 92 naturally occurring elements. Finally, the mass of sulfur needed to produce four grams of sulfur dioxide is 1.99 grams.An element is defined as a pure substance that cannot be decomposed (broken down) into simpler substances.įor example, if you heat nitrogen gas it will get hotter, but it won't break down (decompose) into anything simpler than nitrogen. If we round off to two decimal places, we get 1.99 grams. We get a mass of sulfur of 1.98772 grams, and here I’ve chosen two decimal places. And we know that the molar mass of sulfur is 32.06 grams per mole. We can plug the mole value for sulfur we have just calculated in for the number of moles. Let’s clear a bit of space so that we can do this calculation. We will use the same equation as earlier, this time rearranged so that mass is the subject of the formula. Let’s now convert this mole value of sulfur to a mass value. We need 0.062 moles of sulfur to produce 0.062 moles of sulfur dioxide. And we see that it is the same number of moles. Now we can relate the moles of SO2 we have just calculated, 0.062, to determine the moles of sulfur that is needed. We know from our balanced equation that one mole of sulfur produces one mole of SO2. If we take the mass given to us divided by the molar mass we have just calculated, we get a number of moles of sulfur dioxide of 0.062 moles. The next step, we said, was to determine the number of moles of SO2. So for now, let’s keep the three decimal places. We have not been asked for a specific number of significant figures in this calculation. But there are two oxygen atoms, so we multiply 15.999 by two. From the periodic table, we get 32.06 as the molar mass of sulfur and 15.999 as the molar mass for oxygen. The first step, we said, was to determine the molar mass of SO2. And using this and the number of moles we just calculated, we can calculate the mass of sulfur needed to produce four grams of sulfur dioxide. We could then work out the molar mass of sulfur from the periodic table. From this, we could then determine the number of moles of sulfur needed according to the mole ratio of the equation. If we can work out the molar mass of SO2, we can then use its mass and molar mass together to determine its number of moles. So our first step is to try determine the number of moles for one of the substances. We said we can only relate data from two different substances using the coefficients to determine relative number of moles. We are not given any other data, and we cannot directly determine the mass of sulfur needed from the four grams of sulfur dioxide to be produced. So under sulfur, we could write mass equals question mark. We are also asked what the mass of sulfur is that is needed to produce this four grams of sulfur dioxide. ![]() We are told that four grams of sulfur dioxide are needed to be produced, so we can write this bit of information under SO2. Using the coefficients, we can use the moles of one of the substances to determine the moles of another substance produced or needed.Īt this point, we do not have any more values. And in this case, the stochiometric coefficients are one is to one is to one. We have said that the equation is already balanced. The reaction is an example of a combination reaction because more than one reactant is combining together to form a new product. The balanced equation is S solid plus O2 gas reacting to form SO2 gas. In this reaction, we have sulfur, symbol S, reacting with oxygen gas, O2, to produce sulfur dioxide, SO2, which is also a gas under standard conditions. ![]() What is the mass of sulfur needed to produce four grams of sulfur dioxide? Sulfur burns in oxygen to form sulfur dioxide.
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