8. A chemist burns 160.0 g of Al in 234.78 g of oxygen to produce aluminum...
8. A chemist burns 160.0 g of Al in 234.78 g of oxygen to produce aluminum oxide. She produces 260.0g of solid aluminum oxide. Write a balanced equation for this reaction. Calculate the percent yield. (3 pts)
1. A chemist burns 160.0 g of Mg in excess air to produce aluminum oxide, MgO. She produces 200.0 g of solid Magnesium oxide. Write a balanced equation for the reaction. 2Mg(s)+O2(g)→2MgO(s) Determine the theoretical yield of MgO Determine the percent yield. 2. How many molecules of calcium phosphate are equivalent to 2.75 moles have? Please solve it urgently, Thank you so much
When exposed to air, aluminum metal, Al, reacts with oxygen, O2, to produce a protective coating of aluminum oxide, Al2O3, which prevents the aluminum from rusting underneath. The balanced reaction is shown here: 4Al+3O2→2Al2O3 In Part A, we saw that the theoretical yield of aluminum oxide is 1.90 mol . Calculate the percent yield if the actual yield of aluminum oxide is 1.18 mol .
Question 5 Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al(s) + 302 (g) → 2A1203 (s) The maximum amount of A1203 that can be produced from 2.5 g of Al and 2.5 g of O2 is 5.0 ③ 4.7 3 9.4 * 5.3 * 7.4 Question 3 -/1 The combustion of ammonia in the presence of excess oxygen yields NO2 and H20: 4 NH3(g) + 7 02 (g) → 4NO2(g) + 6H20 (g)...
When exposed to air, aluminum metal, Al, reacts with oxygen, O2, to produce a protective coating of aluminum oxide, Al2O3, which prevents the aluminum from rusting underneath. The balanced reaction is shown here: 4Al+3O2→2Al2O3 a. What is the theoretical yield of aluminum oxide if 1.60 mol of aluminum metal is exposed to 1.50 mol of oxygen?
22. Consider the reaction: solid aluminum and oxygen gas react to form solid aluminum oxide. a. Write and balance the equation. b. How many moles of aluminum are required to react with 47.2 grams of oxygen? c. If 14.0 g of aluminum reacts with oxygen gas, how many grams of aluminum oxide will form? d. How many atoms of aluminum are started with in part c? e. If only 19.7 g of aluminum oxide formed in the reaction from part...
Aluminum oxide (Al2O3) is produced according to the following equation. 4 Al(s) + 3 O2(g) → 2 Al2O3(s) If the reaction occurs with an 82.4% yield, what mass of aluminum should be reacted with excess oxygen to produce 45.0 grams of Al2O3? a. 54.6 g Al b. 37.9 g Al c. 35.1 g Al d. 23.8 g Al e. 28.9 g Al How do we solve this problem
The compound C7H4N306, burns explosively with oxygen to produce CO2, water, and N2- Write a balanced chemical equation for this reaction and calculate the mass of oxygen required (in grams) to burn 100 g of this compound.
A 0.241 g piece of solid aluminum reacts with gaseous oxygen from the atmosphere to form solid aluminum oxide. In the laboratory, a student weighs the mass of the aluminum oxide collected from this reaction as 0.204 g. Part 1 The 0.241 g solid aluminum is the __________. --Choose one: A. limiting reagent B. theoretical yield C. percent yield D. excess reagent E. actual yield Part 2 The 0.204 g aluminum oxide is the __________. --Choose one: A. limiting reagent...
A sample of 4.78 g of aluminum completely reacts with oxygen to form aluminum oxide. Write the balanced chemical equation for the reaction.