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How may grams of oxygen are required to burn 13.50 grams of acetylene?
To burn 1 mole of acetylene (C2H2), 3 moles of oxygen (O2) are required. The molar mass of acetylene is 26.04 g/mol and of oxygen is 32.00 g/mol. First, convert 13.50g acetylene to moles, calculate the moles of oxygen required, and then convert back to grams to find the mass of oxygen needed.
How many moles of oxygen are required to react completely with 1.0 mole of c2h2?
2C2H2 + 5O2 ---->4CO2 + 2H2O so 1 mole of acetylene (ethyne) reacts with 2.5 moles of oxygen. Answer 2.5 moles
How many mols of O2 are needed to completely react with 7 mols of C2H2?
I have already balanced - 2C2H2+5O2->4CO2+2H2O what do I do next? 2 moles acetylene--------------5 moles oxygen O2 7 moles acetylene--------------x moles oxygen O2 x = 7 x 5/2 = 17,5
How many moles of oxygen are needed to completely react with 6 moles of hydrogen?
The balanced chemical equation for the reaction between hydrogen and oxygen is: 2H2 + O2 -> 2H2O This equation shows that 1 mole of O2 reacts with 2 moles of H2. So, to completely react with 6 moles of H2, you would need 3 moles of O2.
What is the mass of CO2 and H2O produced after combusting 100 g of acetylene?
The balanced chemical equation for the combustion of acetylene (C2H2) is 2C2H2 + 5O2 -> 4CO2 + 2H2O. From the equation, for every 2 moles of acetylene combusted, 4 moles of CO2 and 2 moles of H2O are produced. Since the molar mass of acetylene is 26 g/mol, 100 g of acetylene is equivalent to 100/26 = 3.85 moles. Therefore, 3.85 moles of acetylene combustion would produce 7.7 moles of CO2 and 3.85 moles of H2O.
How may grams of oxygen are required to burn 13.50 grams of acetylene?
To burn 1 mole of acetylene (C2H2), 3 moles of oxygen (O2) are required. The molar mass of acetylene is 26.04 g/mol and of oxygen is 32.00 g/mol. First, convert 13.50g acetylene to moles, calculate the moles of oxygen required, and then convert back to grams to find the mass of oxygen needed.
How many moles of Co2 will be produced from the reaction of three moles of acetylene with excess oxygen?
Since acetylene (C2H2) has a stoichiometry of 2 moles of acetylene to produce 2 moles of CO2, three moles of acetylene would produce 3 moles of CO2. The reaction with excess oxygen ensures that all the acetylene is fully converted to CO2.
How many moles of oxygen are required to react completely with 1.0 mole of c2h2?
2C2H2 + 5O2 ---->4CO2 + 2H2O so 1 mole of acetylene (ethyne) reacts with 2.5 moles of oxygen. Answer 2.5 moles
How many moles of oxygen are needed to burn 7.0 mols of phosphorus?
8,75 moles of oxygen are needed.
How many mols of O2 are needed to completely react with 7 mols of C2H2?
I have already balanced - 2C2H2+5O2->4CO2+2H2O what do I do next? 2 moles acetylene--------------5 moles oxygen O2 7 moles acetylene--------------x moles oxygen O2 x = 7 x 5/2 = 17,5
How many moles of oxygen are needed to completely react with 6 moles of hydrogen?
The balanced chemical equation for the reaction between hydrogen and oxygen is: 2H2 + O2 -> 2H2O This equation shows that 1 mole of O2 reacts with 2 moles of H2. So, to completely react with 6 moles of H2, you would need 3 moles of O2.
Acetylene gas C2H2 reacts with oxygen If 2 moles of acetylene react completely with oxygen how many grams of carbon dioxide are produced?
First you need to work out the balanced equation. 2C2H2 + 5O2 -----> 4CO2 + 2H2O From this we see that 2 moles of acetylene produces 4 moles of carbon dioxide. 1 mole of carbon dioxide is 12 + 16 + 16 = 44g (adding the mass numbers of the component elements). If 1 mole = 44g then 4 mole = 176g
If 4 moles of hydrogen is completely oxidized with oxygen how many moles of oxygen will be consumed?
0. Hydrogen doesn't "reackt" to form Nitrogen Monoxide.
What is the mass of CO2 and H2O produced after combusting 100 g of acetylene?
The balanced chemical equation for the combustion of acetylene (C2H2) is 2C2H2 + 5O2 -> 4CO2 + 2H2O. From the equation, for every 2 moles of acetylene combusted, 4 moles of CO2 and 2 moles of H2O are produced. Since the molar mass of acetylene is 26 g/mol, 100 g of acetylene is equivalent to 100/26 = 3.85 moles. Therefore, 3.85 moles of acetylene combustion would produce 7.7 moles of CO2 and 3.85 moles of H2O.
How many moles of O2 are needed to burn 1.35mol of C8H18?
16,875 moles of oxygen are needed.
How many moles of oxygen are needed to react completely with 2.3 moles of H2S?
The balanced chemical equation for the reaction between oxygen (O2) and hydrogen sulfide (H2S) is: 2H2S + 3O2 -> 2SO2 + 2H2O From the equation, it is a 3:2 ratio of O2 to H2S. Therefore, if 2.3 moles of H2S are present, (2.3 moles H2S) * (3 moles O2 / 2 moles H2S) = 3.45 moles of O2 are needed.
How many moles of oxygen are necessary to react completely with 4 moles of propane?
For the reaction of propane (C3H8) with oxygen (O2), the balanced equation is: C3H8 + 5O2 -> 3CO2 + 4H2O. This means that 5 moles of O2 are required to react completely with 1 mole of propane (C3H8). Therefore, to react completely with 4 moles of propane, you would need 20 moles of O2.
