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The chemical formula of carbon dioxide is CO2. This shows that each molecule of carbon dioxide contains two oxygen atoms. The formula mass is about* [12 + (2 X 16)] or 44. 75/44 is about 1.7; therefore the specified amount of carbon dioxide is that many moles of the gas. Oxygen normally exists as diatomic molecules, so that the number of molecules of oxygen gas required is the same as the number of moles of carbon dioxide produced. This number is about 1.7 times Avogadro's number, or about 1.02 X 1024.
*The approximate Atomic Mass of carbon is 12 and that of oxygen is 16.
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There are 3 grams of magnesium and 2 grams of oxygen if 4 grams of magnesium oxide is produced and all of the magnesium was used up how many grams of oxygen are left?
If 3 grams of magnesium are used to form 4 grams of magnesium oxide, then 1 gram of oxygen is used in the reaction. This means 1 gram of oxygen remains unused.
How many molecules of glucose are produced by each cycle of the light reaction?
There are no glucose molecules produced in the light reaction. The light reaction produces ATP and NADPH, which are used in the Calvin cycle to produce glucose from CO2.
How many grams of strontium chloride are produced by the reaction?
The amount of strontium chloride produced in a reaction would depend on the specific reaction involved and the stoichiometry of the reaction. To calculate the grams produced, you would need to know the balanced chemical equation, the amount of the starting materials used, and use stoichiometry to determine the amount of strontium chloride produced.
If 250.0 g of Fe2O3 are used how many grams of iron can be produced?
To determine how many grams of iron can be produced from 250.0 g of Fe₂O₃, we first need to use the molar mass of Fe₂O₃, which is approximately 159.69 g/mol. The balanced chemical reaction for the reduction of Fe₂O₃ to iron is: Fe₂O₃ → 2 Fe + 1.5 O₂. From the stoichiometry of the reaction, 1 mole of Fe₂O₃ produces 2 moles of Fe. Thus, 250.0 g of Fe₂O₃ corresponds to about 1.56 moles, yielding approximately 3.12 moles of Fe, which is about 174.0 g of iron.
If 507 g were used up in the reaction Fe?
To determine how many grams of iron (Fe) were used in a reaction where 507 g were consumed, we need to know the specific reaction and the stoichiometry involved. If we assume that 507 g represents the mass of iron reacting in a balanced chemical equation, we can simply state that 507 g of Fe was utilized. For accurate calculations or further analysis, details about the reaction and other reactants or products involved would be necessary.
If the first reaction used 0.5 g of copper then how many grams of copper will be produced in the last reaction?
Depends on what the last reaction is. And probably what the first reaction was too. Insufficient information in the question.
How many grams of sodium oxide will be formed is 46 grams of sodium are used in the reaction?
If the reaction is:6 Na + 2 O2 = 2 Na2O + Na2O2This mass is 3,83 g sodium.
There are 3 grams of magnesium and 2 grams of oxygen if 4 grams of magnesium oxide is produced and all of the magnesium was used up how many grams of oxygen are left?
If 3 grams of magnesium are used to form 4 grams of magnesium oxide, then 1 gram of oxygen is used in the reaction. This means 1 gram of oxygen remains unused.
How many molecules of glucose are produced by each cycle of the light reaction?
There are no glucose molecules produced in the light reaction. The light reaction produces ATP and NADPH, which are used in the Calvin cycle to produce glucose from CO2.
Given 18.32 grams of aluminum and excess oxygen how many grams of oxygen are used?
To determine the grams of oxygen used, we need to compare the moles of aluminum with the moles of oxygen in the reaction. The balanced chemical equation for the reaction between aluminum and oxygen is 4Al + 3O2 -> 2Al2O3. Using the molar mass of aluminum (26.98 g/mol) and oxygen (16.00 g/mol), we can calculate that 18.32 grams of aluminum would use 27.27 grams of oxygen in the reaction.
How many grams of strontium chloride are produced by the reaction?
The amount of strontium chloride produced in a reaction would depend on the specific reaction involved and the stoichiometry of the reaction. To calculate the grams produced, you would need to know the balanced chemical equation, the amount of the starting materials used, and use stoichiometry to determine the amount of strontium chloride produced.
The are 6 grams of carbon and 20 grams of oxygen if 22 grams of carbon dioxide are produced and all the carbon is used how many grams of oxygen are left?
If 12 grams of carbon were used to form the 22 grams of carbon dioxide, this implies that 12 grams of oxygen were consumed in the reaction. Since 20 grams of oxygen were initially available, only 8 grams of oxygen are left unused.
How many grams of potassium chlorate would be produced by reacting 500 grams of potassium chlorate with oxygen gas?
The reaction between potassium chlorate and oxygen gas generates potassium chloride and oxygen gas. Therefore, the amount of potassium chlorate produced from the reaction is equal to the amount of potassium chlorate that was used, which is 500 grams.
Sodium will react with oxygen to form sodium oxide Use the formula below to determine how many grams of sodium oxide will be formed if 46 grams of sodium are used in the reaction?
The balanced equation for the reaction is: 4 Na + O2 -> 2 Na2O. From the equation, 4 moles of sodium will react to form 2 moles of sodium oxide. Calculate the molar mass of Na2O (sodium oxide) to find out how many grams will be formed.
If you start a chemical reaction with 20 g of reactants the mass of the products produced will be how many grams?
Following the Law of Conservation of Mass (see link below), there will be 20 grams of products in a reaction of 20 grams of reactions.
Kasu means how many grams?
8 grams is 1 Kasu
If 250.0 g of Fe2O3 are used how many grams of iron can be produced?
To determine how many grams of iron can be produced from 250.0 g of Fe₂O₃, we first need to use the molar mass of Fe₂O₃, which is approximately 159.69 g/mol. The balanced chemical reaction for the reduction of Fe₂O₃ to iron is: Fe₂O₃ → 2 Fe + 1.5 O₂. From the stoichiometry of the reaction, 1 mole of Fe₂O₃ produces 2 moles of Fe. Thus, 250.0 g of Fe₂O₃ corresponds to about 1.56 moles, yielding approximately 3.12 moles of Fe, which is about 174.0 g of iron.
