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How many carbon atoms are contained in 84.3 g of ethyne (c2h2)?
3.90x10^24 atoms To arrive at an answer in units of carbon atoms, first we must cancel out the grams by diving 84.3g C2H2 by the molar mass of C2H2 (26.038g/mol). This molar mass is calculated by adding the masses of 2 carbon atoms (12.011g/mol) and 2 hydrogen atoms (1.008g/mol). This renders units of moles of ethyne. Next multiply by Avagadro's number (6.022x10^23 atoms/mol) to cancel the moles of ethyne and reach atoms of ethyne. Finally, because there are 2 carbon atoms in C2H2, multiply by 2 atoms Carbon/1 atom C2H2 to reach the final answer of 3.90x10^24 atoms of Carbon. This answer has been rounded to three significant figures because the lowest known value of significant figures throughout the calculations was three (84.3). The entire process is as follows: 84.3g C2H2 x (1 mol C2H2)/(26.038 g C2H2) x (6.022x10^23 atoms C2H2)/(1 mol C2H2) x (1 atoms C2H2)/(2 atom C) = 3.90x10^24 atoms C
How many grams of C2H2 will be produced if 7 g of Ca(OH)2 are also produced in the following reaction CaC2 plus 2H2O C2H2 plus Ca(OH)2?
CaC2 + 2H2O ==> C2H2 + Ca(OH)2moles of C2H2 produced = moles of Ca(OH)2 produced (1:1 mole ratio is the stoichiometry)moles of Ca(OH)2 produced = 7 g x 1mol/74.1 g = 0.0945 molesmoles C2H2 = 0.0945 molesgrams C2H2 = 0.0945 moles x 26 g/mole = 2.46 grams = 2 grams to 1 sig fig
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 grams of carbon dioxide are produced from the combustion of 1.3 moles of acetylene C2H2?
The balanced chemical equation for the combustion of acetylene is: 2C2H2 + 5O2 → 4CO2 + 2H2O. This means 2 moles of C2H2 produce 4 moles of CO2. Therefore, 1.3 moles of C2H2 will produce 2.6 moles of CO2, which is equivalent to approximately 84.8 grams of CO2.
Is c2h2 charged?
No, C2H2 (acetylene) is a neutral molecule. It consists of two carbon atoms and two hydrogen atoms, with no overall charge.
How many carbon atoms are contained in 84.3 g of ethyne (c2h2)?
3.90x10^24 atoms To arrive at an answer in units of carbon atoms, first we must cancel out the grams by diving 84.3g C2H2 by the molar mass of C2H2 (26.038g/mol). This molar mass is calculated by adding the masses of 2 carbon atoms (12.011g/mol) and 2 hydrogen atoms (1.008g/mol). This renders units of moles of ethyne. Next multiply by Avagadro's number (6.022x10^23 atoms/mol) to cancel the moles of ethyne and reach atoms of ethyne. Finally, because there are 2 carbon atoms in C2H2, multiply by 2 atoms Carbon/1 atom C2H2 to reach the final answer of 3.90x10^24 atoms of Carbon. This answer has been rounded to three significant figures because the lowest known value of significant figures throughout the calculations was three (84.3). The entire process is as follows: 84.3g C2H2 x (1 mol C2H2)/(26.038 g C2H2) x (6.022x10^23 atoms C2H2)/(1 mol C2H2) x (1 atoms C2H2)/(2 atom C) = 3.90x10^24 atoms C
How many moles are contained in 25.0 g of C6H12O6?
Avogadro's constant expresses the number of elementary entities per mole of substance and it has the value 6.02 × 1023 . Thus there will be 2.5 times Avogadro's constant molecules of C6H12O present. And as each molecule contains 12 atoms of Hydrogen The number of atoms of Hydrogen present will be 12 times the product of 2.5 times Avogadro's constant. = 1.806 * 1025 atoms of hydrogen.
How many moles of CO2 are produced when 2.1 mol of C2H2 react?
How many moles of CO2 are produced when 2.1 mol of C2H2 react?
How many grams of C2H2 will be produced if 7 g of Ca(OH)2 are also produced in the following reaction CaC2 plus 2H2O C2H2 plus Ca(OH)2?
CaC2 + 2H2O ==> C2H2 + Ca(OH)2moles of C2H2 produced = moles of Ca(OH)2 produced (1:1 mole ratio is the stoichiometry)moles of Ca(OH)2 produced = 7 g x 1mol/74.1 g = 0.0945 molesmoles C2H2 = 0.0945 molesgrams C2H2 = 0.0945 moles x 26 g/mole = 2.46 grams = 2 grams to 1 sig fig
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 grams of carbon dioxide are produced from the combustion of 1.3 moles of acetylene C2H2?
The balanced chemical equation for the combustion of acetylene is: 2C2H2 + 5O2 → 4CO2 + 2H2O. This means 2 moles of C2H2 produce 4 moles of CO2. Therefore, 1.3 moles of C2H2 will produce 2.6 moles of CO2, which is equivalent to approximately 84.8 grams of CO2.
Is c2h2 charged?
No, C2H2 (acetylene) is a neutral molecule. It consists of two carbon atoms and two hydrogen atoms, with no overall charge.
How many moles of acetylene (C2H2) are needed to completely react with 12 moles of oxygen?
The balanced chemical equation for the combustion of acetylene is: 2 C2H2 + 5 O2 → 4 CO2 + 2 H2O From the equation, 2 moles of acetylene react with 5 moles of oxygen. Therefore, 12 moles of oxygen would react with 12/5 * 2 = 4.8 moles of acetylene.
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
The empirical formula for acetylene?
Acetylene is C2H2 so its emperical formula is C1H1.
How much co2 is produced when 30000g of c2h2 burns completely?
2C2H2 + 5O2 ------------->2H2O + 4CO21 mole Of C2H2 = 26.04g, O2 = 32g, H2O = 44.01g, CO2 = 18.01g2moleC2H2 -------------> 4moleCO22x(26.04g) -------------> 4x(18.01g)52.08 g C2H2 ---------> 176.04 g CO230000g C2H2 ---------> ?? =176.04x30000g/52.08 =101405.53 gAnswer=101405.53 gram of CO2
What is a chemical formula of acetylene?
Acetylene has the chemical formula pf C2H2.
