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If 5.58 g of iron react with sulfur to produce 8.79 g of iron sulfide what is the mass of reacting sulfur?
To find the mass of reacting sulfur, we can use the law of conservation of mass, which states that the mass of the reactants equals the mass of the products. Here, the mass of iron sulfide produced (8.79 g) is the sum of the mass of iron (5.58 g) and the mass of sulfur. Thus, the mass of sulfur can be calculated as: Mass of sulfur = Mass of iron sulfide - Mass of iron Mass of sulfur = 8.79 g - 5.58 g = 3.21 g. Therefore, the mass of reacting sulfur is 3.21 g.
How many ounces would 12.30 moles of sulfur hexafluoride weigh?
To find the weight in ounces, you need to know the molar mass of sulfur hexafluoride (SF6), which is approximately 146.06 g/mol. In this case, 12.30 moles of SF6 would weigh approximately 1794.3 grams. To convert this to ounces, you would divide by 28.35 (1 ounce ≈ 28.35 grams), giving you around 63.3 ounces.
Which one has a greater atomic mass fluorine or carbon?
Fluorine has a greater atomic mass than carbon. Carbon has an atomic mass of approximately 12 atomic mass units (amu) while fluorine has an atomic mass of approximately 19 amu.
What is the Atomic Mass of fluorine?
The atomic mass number for fluorine is 18.9998, rounded to 19. Most fluorine is 19F but some is 18F with a half-life of 109.77 minutes.
What is the atomic mass of flurine?
Fluorine is a non metal element. Atomic mass of it is 19.
What is the atomic number of sulfur hexafluoride?
There is no "atomic number" associated with Sulfur HexaFluoride. There is an atomic mass associated with the molecule. Just add up the atomic masses of 1 sulfur atom and 6 Fluoride atoms.
What is the percent composition of sulfur in sulfur hexafluoride?
21.95%
What is the percent composition of sulfur in sulfur hexafluoride gas?
Sulfur hexafluoride (SF6) has a molar mass of 146.06 g/mol. The molar mass of sulfur is 32.06 g/mol. To find the percent composition of sulfur in SF6, you would calculate: (32.06 g/mol sulfur / 146.06 g/mol SF6) x 100 = 22.0%. So, sulfur makes up 22.0% of the mass of SF6 gas.
What is the correct formula to find the molar mass of xenon hexafluoride?
The molar mass of xenon hexafluoride (XeF6) can be found by adding the atomic masses of one xenon atom and six fluorine atoms. The atomic mass of xenon is 131.293 u, and the atomic mass of fluorine is 18.998 u. So, the molar mass of XeF6 is approximately 245.29 g/mol.
How many moles of fluorine are in 3.2 grams of xenon hexafluoride?
First, calculate the molar mass of xenon hexafluoride (XeF6). Xenon has a molar mass of 131.29 g/mol and each fluorine atom has a molar mass of 19.00 g/mol. Therefore, the molar mass of XeF6 is 131.29 + (6 * 19.00) = 209.29 g/mol. Next, calculate the number of moles in 3.2 grams of XeF6 by dividing the given mass by the molar mass: 3.2 g / 209.29 g/mol ≈ 0.0153 moles of XeF6. This means that there are about 0.0153 moles of fluorine atoms in 3.2 grams of xenon hexafluoride.
Propose an explanation for the effectiveness of ozone and sulfur hexafluoride to act as greenhouse gases compared to carbon dioxide?
Ozone and sulfur hexafluoride are non-linear molecules with the same number or more mass centers. This gives them additional resonance modes, allowing them to interact with broader ranges of EM radiation.
In SF6 the mass of fluorine per gram of sulfur is 3.55g In the other compound SFx the mass of fluorine per gram of sulfur is 1.18g What is the value of X for the second compound?
1.18 x 3 = 3.55 you need to find the ratio of F to F in each compound. this is the law of multiple proportions stating that the masses of one element which combine with a fixed mass of the second element are in a ratio of whole numbers. here, in this case F would be the "one element" and S would be the "fixed mass", the ratio of F6 to Fx = 3:1 therefore x would be 2 since there is less F in SFx and the ratio is 3:1. divide 6 by 3 and you get 2.
What is the mole mass for xenon hexafluoride?
The molar mass of xenon hexafluoride (XeF6) is 245.28 g/mol.
How much fluorine in grams was formed when the mass ratio of sodium to fluorine in sodium fluoride is 1 to 21 to 1 A sample of sodium fluoride produced 27point7 grams of sodium upon decomposition?
To find the mass of fluorine produced, first calculate the mass of sodium fluoride: 27.7 grams of sodium / (1 part sodium / 1 part sodium fluoride) = 27.7 grams of sodium fluoride Now, since the ratio of sodium to fluorine in sodium fluoride is 1:2 (1 part sodium to 2 parts fluorine), the mass of fluorine is 27.7 grams / 2 = 13.85 grams.
How much sulfur dioxide can be produced from 64kg of sulfur?
The molar mass of sulfur is 32 g/mol and the molar mass of sulfur dioxide is 64 g/mol. Thus, from 64 kg of sulfur, you can produce 1280 kg (1.28 metric tons) of sulfur dioxide using stoichiometry.
What is the Atom mass in Fluorine?
Fluorine is a metal element. Atomic Mass of it is 19.
How many ounces would 12.30 moles of sulfur hexafluoride weigh?
To find the weight in ounces, you need to know the molar mass of sulfur hexafluoride (SF6), which is approximately 146.06 g/mol. In this case, 12.30 moles of SF6 would weigh approximately 1794.3 grams. To convert this to ounces, you would divide by 28.35 (1 ounce ≈ 28.35 grams), giving you around 63.3 ounces.
