Chemical analysis of an unknown compound gives a molar mass of 334 g/mol and a percentage...

Chemical analysis of an unknown compound gives a molar mass of

334 g/mol and a percentage composition of 75.42% carbon, 6.63% hydrogen,

8.38% nitrogen, and the rest is oxygen. Calculate the empirical and molecular

formulas for the unknown compound.

2.) Write a balanced chemical equation for the complete combustion of

pentane (C5H12). If 100.00 g of pentane are combusted in excess O2, what mass

of CO2 would be released to the atmosphere?

Expert Solution

queen_honey_blossom answered 9 months ago

An unknown compound with a molar mass of 176 g/mol is analyzed and determine to consist...

An unknown compound with a molar mass of 176 g/mol is analyzed and determine to consist of 40.91 mass percent carbon, 4.58 mass percent hydrogen and the remainder oxygen. What are the empirical and molecular formulas for this compound

A compound has a molar mass of 100 g/mol and the percent composition (by mass) of...

A compound has a molar mass of 100 g/mol and the percent composition (by mass) of 65.45% C, 5.45% H, and 29.09% O. Determine the empirical formula and the molecular formula.

When 2.65 g of an unknown weak acid (HA) with a molar mass of 85.0 g/mol...

When 2.65 g of an unknown weak acid (HA) with a molar mass of 85.0 g/mol is dissolved in 250.0 g of water, the freezing point of the resulting solution is -0.257 ∘C.

A compound with the empirical formula of CH4O and a molar mass of 32 g/mol has...

A compound with the empirical formula of CH4O and a molar mass of 32 g/mol has a molecular formula of:

A compound with the empirical formula CH2 has a molar mass of 98 g/mol. What is...

A compound with the empirical formula CH2 has a molar mass of 98 g/mol. What is the molecular formula for this compound? 2-A compound is 54.53% C, 9.15% H, and 36.32% O by mass. What is its empirical formula? 3-The molecular mass of the compound is 132 amu. What is the molecular formula? 4What is the empirical formula of a compound composed of 3.25% hydrogen (H), 19.36% carbon (C), and 77.39% oxygen (O) by mass? 5What is the empirical formula...

1. The molar mass of a compound is 126 g/mol, and it's empirical formula is C2H2O....

1. The molar mass of a compound is 126 g/mol, and it's empirical formula is C2H2O. What is compound's molecular formula? 2. A compound consist of 26.18g Si and 29.82g O. Calculate its empirical formula? 3. Calculate the empirical formula of the compound that consist of 70.4%F and 29.6%O.

Chem Question - Gases Molar Mass N = 14.01 g/mol Molar Mass H2O = 18.016 g/mol...

Chem Question - Gases Molar Mass N = 14.01 g/mol Molar Mass H2O = 18.016 g/mol Vapor Pressure of Water at 25 C is 23.76 torr Vapor Pressure of Water at 65 C is 187.54 torr (Show all work and calculations, include units in answer. If calculations must be used in several parts, rounding should be made to 6 decimal points to ensure accuracy. Final Answers can be rounded to 3 decimal points.) A syringe filled with air can be...

20.26 grams of unknown 1 (with molar mass 203.67 g/mol) was dissolved in 182.7 mL of...

20.26 grams of unknown 1 (with molar mass 203.67 g/mol) was dissolved in 182.7 mL of ethylene glycol in a calorimeter. What change in temperature would the solution experience as a result of this dissolution? Assume the solution has the same specific heat capacity as pure ethylene glycol. The density of ethylene glycol is 1.11 g/cm3. The ∆Hdissolution for unknown 2 is 124.1 kJ/mol unknown 1.

An organic compound, containing only C, H, N, has a molar mass of 162 g/mol. The...

An organic compound, containing only C, H, N, has a molar mass of 162 g/mol. The combustion of 5.64 mg of the compound released 15.30 mg CO2 and 4.39 mg H2O. What is the molecular formula of this organic compound?

a). Calculate the molar mass in g/mol of the following compound (ammonium dichromate): (NH4)2Cr2O7 b). Calculate...

a). Calculate the molar mass in g/mol of the following compound (ammonium dichromate): (NH4)2Cr2O7 b). Calculate the mass, in g, of the following: 0.158 mol IF5 (iodine pentafluoride) c). Calculate the amount, in moles, of the following: 25.4 g Pb(C2H3O2)2 (lead (II) acetate) Professors Note: Make sure that you give your answer in a clear and well-reasoned manner, providing necessary explanation on how did you come up with it. d). Calculate the percent by mass of C, H, and O...

Question