The gram molecular mass of carbon dioxide is 44.01. Therefore, 418 grams contains 418/44.01 or 9.50 moles, to the justified number of significant digits.
To produce 1 mole of urea, 1 mole of carbon dioxide is needed. The molar mass of urea is 60 grams/mol, and the molar mass of carbon dioxide is 44 grams/mol. Therefore, to produce 125 grams of urea, 125 grams/60 grams/mol = 2.08 moles of urea is needed. This means 2.08 moles of carbon dioxide is needed, which is 2.08 moles * 44 grams/mol = 91.52 grams of carbon dioxide needed.
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.
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)
Balanced equation. C + O2 -> CO2 22.2 grams carbon (1 mole C/12.01 grams)(1 mole CO2/1 mole C) = 1.85 moles carbon dioxide produced -------------------------------------------------
To determine the mass of carbon monoxide in 2.55 moles, we first find the molar mass of CO, which is 28.01 g/mol. Then, we multiply the molar mass by the number of moles: 28.01 g/mol * 2.55 mol = 71.53 grams of CO in 2.55 moles of the compound.
To calculate the number of moles of carbon dioxide in 19 grams, divide the given mass by the molar mass of carbon dioxide, which is approximately 44 grams/mol. Therefore, 19 grams of carbon dioxide is equal to 19/44 ≈ 0.43 moles.
Look up the molecular weight of carbon dioxide in the periodic table. The formula for carbon dioxide is CO2, which means one atom of carbon and two atoms or oxygen per molecule of carbon dioxide. Carbon has molecular weight of 12. Oxygen molecular weight is 16. Total 12+16+16= 44 11 grams/44 grams/mole=0.25 moles of carbon The grams of water and combustion of 7.5 grams are totally irrelevant. They are only given to possibly confuse you.
To produce 1 mole of urea, 1 mole of carbon dioxide is needed. The molar mass of urea is 60 grams/mol, and the molar mass of carbon dioxide is 44 grams/mol. Therefore, to produce 125 grams of urea, 125 grams/60 grams/mol = 2.08 moles of urea is needed. This means 2.08 moles of carbon dioxide is needed, which is 2.08 moles * 44 grams/mol = 91.52 grams of carbon dioxide needed.
To calculate the number of moles in 66 grams of carbon dioxide, we need to divide the given mass by the molar mass of carbon dioxide. The molar mass of carbon dioxide is approximately 44 grams per mole. Therefore, 66 grams of carbon dioxide is equal to 66/44 ≈ 1.5 moles.
The answer is 3,99 moles of carbon dioxide.
The answer is 3,99 moles of carbon dioxide.
0.1 moles There is one carbon and two oxygens 1 x 0.1 = 0.1
211g of carbon dioxide are equal to 4,794 moles.
85.636 grams carbon (1 mole C/12.01 grams) = 7.1304 moles of carbon ---------------------------------
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.
First, convert the mass of carbon dioxide to grams by dividing by 1000: 220 mg = 0.22 g. Next, use the molar mass of carbon dioxide (44 g/mol) to calculate the number of moles: 0.22 g / 44 g/mol = 0.005 moles of carbon dioxide.
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)