Cobalt (III) fluoride is reacted with sulfur tetrafluoride to form sulfur hexafluoride and cobalt (II) fluoride. Calculate the amount of cobalt (III) fluoride needed to form 5.95 g of sulfur hexafluoride.   Atomic Mass: Co: 58.933 g/mol F: 18.998 g/mol S: 32.065 g/mol

An analytical chemist measures the amount Elements E₁ and E₂ in four samples of an unknown Substance X: mass mass sample of E₁ of E₂ 12.1 g 13.9 g 11.3 g 12.7 g 13.6 g 15.4 g 6.6 g 7.5 g Using this information, answer the questions in the table below. 1 2 3 4 It's known that X contains no elements other than E, and E₂. Is X a pure substance or a mixture? If you don't have enough information to decide, choose can't decide. If you said X is a pure substance, calculate the mass of Element E, the analytical chemist would find in a new 10.0 g sample of X. Round your answer to 2 significant digits. O pure substance O mixture O (can't decide) 0 X S s

Let’s put the above values into the formula: V1 = 8.00 mol.L-1 × 2.42 L13.0 mol.L-1V1 = 8.00 mol.L-1 × 2.42 L13.0 mol.L-1V1 = 8.00 × 2.42 L13.0V1 = 1.4892 LV1 = 1.49 L This part is little confusing

An analytical chemist measures the amount of Elements E₁ and E₂ in four samples of an unknown Substance X: mass mass of E₂ sample of E₁ 1 1 2 3 4 3.7 g 30.3 g It's known that X contains no elements other than E₁ and E₂. 4.6 g 15.4 g 3.2 g 25.8 g 3.4 g 27.6 g Using this information, answer the questions in the table below. Is X a pure substance or a mixture? If you don't have enough information to decide, choose can't decide. If you said X is a pure substance, calculate the mass of Element E₁ the analytical chemist would find in a new 10.0 g sample of X. Round your answer to 2 significant digits. OOO pure substance mixture (can't decide) Πε g x10 X Ś

The formula for sulfur hexafluoride is . a. How many molecules are in 2.24 grams of sulfur hexafluoride? ____molecules b. What is the mass in grams of 7.72 x 10^22 molecules of sulfur hexafluoride? ____grams

A classic SUV features a 194 L gas tank. Assuming a molecular formula of C8H18 for gasoline and complete combustion of the gasoline with O2 to form CO2 and H2O, calculate the amount of O2 in kilograms consumed per tank of gasoline. Assume a density of 780 g/L for the gasoline.   Atomic Mass: C: 12.011 g/mol H: 1.008 g/mol O: 15.999 g/mol   Round your answer to 2 decimal places.

221.89 g/mol 2IF5(0) 38.00 g/mol 5 F2(9) 253.8 g/mol I2(s) 5. ) a. What is the mass (in grams) of fluorine gas that can be produced from 85.00 grams of iodine pentafluoride? b. Calculate the percent yield if a student uses 85.00 grams of iodine pentafluoride, but obtains 23.20 grams of fluorine gas.

In air, nitric oxide gas reacts with oxygen to produce nitrogen dioxide, which appears brown in color: 2 NO(g) + 0,(9) = 2NO,(g) What mass in grams of nitrogen dioxide would be produced by the complete reaction of 0.551 grams of nitric oxide gas? MacBook Air SC 80 F2 F4 F6 F7 @ 2# $ % & 1 2 3 4 5 Q W E R Y A S F G

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An unknown compound has the formula CH₂Oz. You burn 0.1095 g of the compound and isolate 0.2674 g of CO2 and 0.1094 g of H₂O. What is the empirical formula of the compound? If the molar mass is 72.1 g/mol, what is the molecular formula? (Enter the elements in the order: C, H, O.) Empirical formula: Molecular formula: Cengage Learning Cengage Technical Support