(1)Aluminum reacts with oxygen to produce aluminum oxide according to the following reaction:
4Al(s) + 3O2(g) → 2Al2O3(s)
Calculate the moles of Al2O3 produced when the reaction is performed with 31.06 g of each reactant.
(2)Nitrogen dioxide reacts with water to produce nitric acid and nitrogen monoxide according to the following reaction:
3NO2(g) + H2O(g) → 2HNO3(g) + NO(g)
Calculate the moles of nitric acid produced when 46.79 grams of each reactant is used.
(3)Ammonia reacts with oxygen to produce nitrogen monoxide and water according to the following equation:
4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(l)
Calculate the moles of water produced in this reaction when 88.82 grams of each reactant are used.
(4)A rocket can be powered by the reaction of dinitrogen tetroxide (N2O4) and hydrazine (N2H4):
N2O4(l) + 2N2H4(l) → 3N2(g) + 4H2O(g)
A rocket was designed to hold 4.16 kilograms dinitrogen tetroxide and excess hydrazine. How much nitrogen gas in grams would be produced in this rocket?
Aluminum reacts with oxygen gas to produce aluminum oxide. How many moles of aluminum oxide would you expect to produce if you reacted 14.5 moles of oxygen gas with excess aluminum? 4Al +3O2 --> 2Al2O3 14.5 mol O2 x 4 mol Al /
Can you tell me if these are right please? When 2.50g of copper reacts with oxygen the copper oxide product has a mass of 2.81g. What is the simplest formula of the copper oxide. I got Cu2O (copper (I) oxide). Aluminum and oxygen
1. Aluminum reacts with oxygen to produce aluminum oxide which can be used as an adsorbent, desiccant or catalyst for organic reactions. 4Al(s) + 3O2(g) → 2Al2O3(s) A mixture of 82.49 g of aluminum ( Picture = 26.98 g/mol)
In this balanced equation 4Al + 3O2 = 2Al2O3. When 0.54 mole aluminum is reacted in a closed container with 7.80 g oxygen, how many grams of aluminum oxide can form. Please show steps to work out. Thanks
Aluminum cookware is reffered ti as "anodized aluminum". The anodizing process puts a layer of aluminum oxide on the aluminum, protecting it from corrosion. Consider the reaction of 10.00 grams of aluminum with 10.00 grams of
A 4.78-g sample of aluminum completely reacts with oxygen to form 6.67 g of aluminum oxide Use this data to calculate the mass percent composition of aluminum in aluminum oxide. (Sorry need help with this!)