2. Dimethylamine burns in oxygen according to the following equation: 4 C2H7N + 15 O2 →...

Question

Question

2. Dimethylamine burns in oxygen according to the following equation: 4 C2H7N + 15 O2 → 8 CO2 + 14 H2O + 2 N2

(a) How many liters of O2 at 35 °C and 0.840 atm will be needed to burn 7.70 L of C2H7N at 35 °C and 0.840 atm?

(b) How many liters of CO2 at 35 °C and 0.840 atm will be produced? Report your answers to parts (a) and (b) to 3 significant figures.

3. Complete combustion of a 0.0100 mol sample of a hydrocarbon, CxHy, gives 0.896 L of CO2 at STP and 0.540 g of H2O.

(a) What is the molecular formula of the hydrocarbon?

(b) What is the empirical formula of the hydrocarbon?

science chemistry

Answer 1

Answer #1

mol C27 N PV RT = (o.0021)(3.8) 217 N o.211 mol 155 Xa.2J 6.9r9 me (0.919)(a.t 21) 3.e MRT 28.27 L 0.5I mo 0.Si) (0,0021) (20

Answer 2

Similar Homework Help Questions

Complete combustion of a 0.0100 mol sample of a hydrocarbon, CxHy, gives 1.792 L of CO2...

Complete combustion of a 0.0100 mol sample of a hydrocarbon, CxHy, gives 1.792 L of CO2 at STP and 1.261 g of H2O. (a) What is the molecular formula of the hydrocarbon? (b) What is the empirical formula of the hydrocarbon?
Methyl ethyl ether burns in oxygen according to the following equation: 2 C3H8O + 9O2 →...

Methyl ethyl ether burns in oxygen according to the following equation: 2 C3H8O + 9O2 → 6CO2 + 8H2O (a) How many liters of O2 at 37 °C and 0.410 atm will be needed to burn 8.01 L of C3H8O at 37 °C and 0.410 atm? (b) How many liters of CO2 at 37 °C and 0.410 atm will be produced? Report your answers to parts (a) and (b) to 3 significant figures.
35a When 4.752 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 16.06...

35a When 4.752 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 16.06 grams of CO2 and 3.289 grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 26.04 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon. 35 part b A 4.079 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 9.273 grams of CO2 and...

Use this balanced equation to answer the following stoichiometry problem. 2C3H18(1) + 25 O2(g) →16 CO2(g)...

Use this balanced equation to answer the following stoichiometry problem. 2C3H18(1) + 25 O2(g) →16 CO2(g) + 18 H2O(g) The molar masses in grams are: C8H18 = 114; O2 = 32; CO, = 44; H20 = 18. If you burn 72.9 g of octane, how many liters at STP of CO2 are produced? O 179 L 129 L 83.5L 115L
6.0 grams hydrocarbon sample were made to react with oxygen gas to produce 17.6 grams of...

6.0 grams hydrocarbon sample were made to react with oxygen gas to produce 17.6 grams of carbon dioxide according to the equation: CxHy(g) + O2(g) ---------- CO2(g) + H20(l) where x = subscript for C, y = subscript for H a. How many grams of C are there in 17.6 grams of CO2? b. How many grams of C are there in the hydrocarbon sample? c. How many moles of C are there in the hydrocarbon sample? d. How many...
Isooctane, C8H18, is the component of gasoline from which the term octane rating derives. A. Write a balanced equation f...

Isooctane, C8H18, is the component of gasoline from which the term octane rating derives. A. Write a balanced equation for the combustion of isooctane to yield CO2 and H2O. B. Assuming that gasoline is 100% isooctane, the isooctane burns to produce only CO2 and H2O, and that the density of isooctane is 0.792 g/mL, what mass of CO2 in kilograms is produced each year by the annual US gasoline consumption of 4.6 x 10^10 L? C. What is the volume...

The balanced equation for the combustion of ethanol into carbon dioxide and water is found below.....

The balanced equation for the combustion of ethanol into carbon dioxide and water is found below.. C2H5OH (l) + 3 O2 (g) ----> 2 CO2 (g) + 3 H2O (l) a.calculate how many moles of oxygen gas are contained in 659 ml sample of oxygen at 1.07 atm and 21 degrees celcius b. a glass of wine contains 9.33g of ethanol. how many moles of oxygen would be needed to burn the ethanol contained in one glass of wine c....
How many liters of oxygen at 23° C and 1.12 atm will be required for the...

How many liters of oxygen at 23° C and 1.12 atm will be required for the combustion of 10.0 g of methane, CH4, according to the chemical reaction below: CH4 (g) + 2 O2 (g) ---> CO2 (g) + 2 H2O (g) When magnesium burns in air, the reaction is described by: 2 Mg (s) + O2 (g) ---> 2 MgO (s) What mass of magnesium will react with 10.8 L of oxygen if the temperature and pressure of the...
If we have C3H8 + 5O2 ---> 3CO2 + 4H2O a) How many liters of oxygen...

If we have C3H8 + 5O2 ---> 3CO2 + 4H2O a) How many liters of oxygen gas are required to react with 7.2 L of C3H8 if both gasses are at STP? b) How many grams of CO2 will be produced from 35 L C3H8 at 15 C and 1.65 atm? c) How many grams of water vapor can be produced when 15 L C3H8 at 15 C and 1.65 atm are reacted with 15 L O2 at -20.0 C...

Under STP conditions, 100.0 mL of an unknown hydrocarbon gas was combusted in excess oxygen. The...

Under STP conditions, 100.0 mL of an unknown hydrocarbon gas was combusted in excess oxygen. The only products of the combustion were 300.0 mL of carbon dioxide and 400.0 mL of water vapor. a. What are the intermolecular forces common to hydrocarbon gases? b. Does the behavior of these gases tend to resemble ideal gas behavior? How might these gases be expected to deviate from this behavior? c. How many moles of carbon dioxide are produced in the combustion? d....