30.8g of iron (approximately) reacted with 13.2g of oxygen will yield 44g of iron(III) oxide (Fe2O3) with 2.8g of oxygen left unreacted. This assumes Atomic Mass numbers of 56 and 16 respectively for iron and oxygen. The actual mass number of iron is 55.847 and oxygen 15.9994 making the figures 30.775g of iron and 13.225g of oxygen with 2.775g of unreacted oxygen. Of course this is an exothermic reaction so will there be a tiny tiny loss of mass in the system as it is converted to heat energy, according to E=MC^2? I'll let you work that one out...
62 grams a+
62 grams a+
An oxygen atom can only be oxidized by some element with an equal or higher electronegativity. So, oxygen can be oxidized by fluorine (e.g., OF2) or by another oxygen atom (e.g., O2).
The chemical formula for Calcium Oxide is CaO. The Atomic weigth of Calcium is 40.078. The Atomic weight of Oxygen is 15.999 The Molecular weight of CaO is therefore 56.077 Thus 100g of CaO would contain (15.999/56.077)*100 = 28.53041353852738 grams of Oxygen and (40.078/56.077)*100 = 71.46958646147262 grams of Calcium.
aluminium nitrate
Sounds like 42.2 grams, but I haven't checked your proportions, are these stoichometric?
32,895 g of triuraniumoctaoxide (U3O8).
2
Sulphur + oxygen = Sulphur Oxide
340 grams
The radium oxide is formed.
62 grams a+
62 grams a+
Magnesium and Oxygen equals Magnesium Oxide (2MgO) 2Mg + O2 --> 2MgO
If 20g of mercury oxide were heated, the combined mass of oxygen and mercury would be 20 grams.
i dont know help :C
adds more oxygen to the engine