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How many grams of oxygen are in 1.851023 formula units of (NH4)2SO4?
Wiki User
∙ 9y ago
This mass is 244,459.10e23 g.
Wiki User
∙ 8y ago
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Why molecular formula of ozone is O3?
O3, with a molecular mass of 48 grams per mole
A compound is formed when 48 grams of carbon 8 grams of hydrogen and 68 grams oxygen combine what is the percent by mass of oxygen?
The percentage of oxygen is 54,84 %.
How many moles of in 320 grams of oxygen?
320 grams of oxygen is the equivalent of 10 moles.
What is 16 grams of oxygen how many moles?
16 grams of oxygen how many moles is 0,5 moles.
If 16g of oxygen contains 1 mole of oxygen atoms calculate the mass of one atom of oxygen in grams?
1
How many moles of (NH4)2SO4 do you have?
0.758 moles of NH3 is the amount of moles in 50 grams of NH42SO4.
Zircon is a mineral with the empirical formula ZrSiO4. What mass of Oxygen is present in 10.0 g of Zircon?
640 grams of Oxygen
He formula for potassium dichromate is KËÃCrËÃOËÈ How many grams of oxygen will be in 2 moles of potassium dichromate?
224 grams of Oxygen will be in 2 moles of Potassium dichromate.
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?
62 grams a+
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.?
62 grams a+
What is a formula for wollastonite?
Wallastonite is a silicate mineral is comprised of calcium, silicon, and oxygen. The molecular formula is CaSi03, with a molecular weight of 116.16 grams per mole.
A sample of a compound contain 1.52 g of Nitrogen and 3.47 g of Oxygen. The molar mass of this compound is between 90 grams and 95 grams. Determine molecular formula and the accurate molar mass.?
A sample of a compound contain 1.52 g of Nitrogen and 3.47 g of Oxygen. The molar mass of this compound is between 90 grams and 95 grams. The molecular formula and the accurate molar mass would be N14O35.
Why molecular formula of ozone is O3?
O3, with a molecular mass of 48 grams per mole
What is the empirical formula of a compound that is 40 percent sulfur and 60 percent oxygen by weight?
We assume 100 grams of compound and change % to grams. Get moles. 40 grams S (1 mole S/32.07 grams) = 1.247 60 grams O (1 mole O/16.0 grams) = 3.75 Now, the smallest mole value, sulfur, is 1. Divide the oxygen mole value by the sulfur mole value. 3.75 mole O/1.247 mole S = 3.00 SO3 ------- is the empirical formula
What is the empirical formula for 16 grams of sulfur reacting with 24 grams of oxygen?
To find empirical formulas, masses of elemental reactants must be changed to gram atoms by dividing the mass by the gram atomic masses of each element. Thus, 16 grams of sulfur constitutes 16/32.06 or 0.50 mole to the justified number of significant digits, and 24 grams of oxygen constitutes 24/15.9994 or 1.50 moles of oxygen to the justified number of significant digits. Therefore, the atomic ratio of oxygen to sulfur in the compound is 1.50/0.50 or 3, and the empirical formula is SO3.
How many grams of oxygen are needed for the complete combustion of the butane in the lighter?
The variables for the formula are incomplete. You would need to know how many grams of butane are put out by the lighter. The molecular weight of butane is 58.12 g/mol, which is also needed to complete the formula.
When the amount of oxygen is limited carbon and oxygen react to form carbon monoxide. How many grams of CO can be formed from 35 grams of oxygen?
When the amount of oxygen is limited, carbon and oxygen react to form carbon monoxide. How many grams of CO can be formed from 35 grams of oxygen?
