5.0 grams CO2 (1mol CO2/44.01g) = 0.11 moles CO2
For this reaction, the stoichiometry indicates that 4 moles of CO2 are produced for every 2 moles of C2H2 reacted. The molar mass of CO2 is approximately 44 g/mol. Therefore, you can calculate the mass of CO2 produced by converting the moles of CO2 into grams.
To determine the grams of CO2 produced from 2.5 moles of O2, we first need to consider the balanced chemical equation for the combustion of a hydrocarbon (e.g., methane): CH4 + 2O2 → CO2 + 2H2O. From this equation, 2 moles of O2 produce 1 mole of CO2. Therefore, 2.5 moles of O2 would produce 1.25 moles of CO2. Since the molar mass of CO2 is approximately 44 grams/mol, 1.25 moles of CO2 corresponds to 55 grams (1.25 moles × 44 g/mol).
To calculate the mass of CO2 produced from 128.00 g of O2, you need to use the balanced chemical equation for the reaction. The molar ratio between O2 and CO2 is 1:2, so if you have 128.00 g of O2, you can calculate the mass of CO2 produced by first converting grams of O2 to moles, then using the mole ratio to find the moles of CO2, and finally converting moles of CO2 to grams.
To calculate the moles of O2 produced, first find the moles of CO2 using its molar mass, which is 44.01 g/mol. Then, use the mole ratio from the balanced equation to find the moles of O2 produced. Finally, multiply the moles of CO2 by the mole ratio to get the moles of O2 produced.
For every 1 mole of CH4 that reacts, 1 mole of CO2 is produced. Therefore, 4 moles of CH4 will produce 4 moles of CO2. To calculate the mass of CO2 produced, you would need to multiply the moles of CO2 by its molar mass (44 g/mole) to get the total mass produced.
To calculate the grams of CO2 produced by burning 22 grams of C3H8, first determine the moles of C3H8 using its molar mass, then use the balanced chemical equation for the combustion of C3H8 to find the moles of CO2 produced, and finally convert moles of CO2 to grams using the molar mass of CO2.
For this reaction, the stoichiometry indicates that 4 moles of CO2 are produced for every 2 moles of C2H2 reacted. The molar mass of CO2 is approximately 44 g/mol. Therefore, you can calculate the mass of CO2 produced by converting the moles of CO2 into grams.
To calculate the mass of CO2 produced from 128.00 g of O2, you need to use the balanced chemical equation for the reaction. The molar ratio between O2 and CO2 is 1:2, so if you have 128.00 g of O2, you can calculate the mass of CO2 produced by first converting grams of O2 to moles, then using the mole ratio to find the moles of CO2, and finally converting moles of CO2 to grams.
To calculate the amount of CO2 produced when burning 34.3 grams of C3H8 (propane), you need to balance the chemical equation for the combustion of C3H8. Since each mole of C3H8 produces 3 moles of CO2, you first convert 34.3 grams of C3H8 to moles, calculate the moles of CO2 produced, and then convert that to grams of CO2.
For every 2 moles of O2 produced, 3 moles of CO2 are used in the reaction. So you need to calculate the moles of O2 produced first using its molar mass, then use the mole ratio to find the moles of CO2 used. Finally, convert the moles of CO2 to grams using its molar mass.
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.
How many moles of CO2 are produced when 2.1 mol of C2H2 react?
To calculate the moles of O2 produced, first find the moles of CO2 using its molar mass, which is 44.01 g/mol. Then, use the mole ratio from the balanced equation to find the moles of O2 produced. Finally, multiply the moles of CO2 by the mole ratio to get the moles of O2 produced.
To find the grams of carbon dioxide produced, first determine the moles of 1-heptanol using its molar mass. Then, use the balanced combustion equation of 1-heptanol to find the moles of CO2 produced. Finally, convert moles of CO2 to grams using its molar mass.
C6H12O6 + 6O2 --> 6CO2 + 6H2O 45 grams C6H12O6 (1 mole C6H12O6/180.156 grams)(6 moles CO2/1 mole C6H12O6)(44.01 grams/1 mole CO2) = 66 grams carbon dioxide produced ==========================
To find the mass of CO2 produced, first calculate the moles of C2H4 using its molar mass. Then, use the balanced equation to determine the moles of CO2 produced per mole of C2H4 reacted. Finally, convert moles of CO2 to grams using the molar mass of CO2.
First write the balance equation: Na2CO3 + 2HNO3 ==> 2NaNO3 + CO2 + H2O Next calculate moles of Na2CO3 used: 7.5 g x 1 mole/106 g = 0.071 moles Na2CO3 Then look at mole ratio of Na2CO3 to CO2 and see that it is 1 to 1 Thus, moles CO2 produced = 0.071 moles Finally, convert moles CO2 to grams of CO2: 0.071 moles x 44g/mole = 3.1 g (to 2 significant figures)