Detonation of nitroglycerin proceeds as follows: 4C3H5N3O9(l)→12CO2(g)+6N2(g)+O2(g)+10H2O(g)4C3H5N3O9(l)→12CO2(g)+6N2(g)+O2(g)+10H2O(g). Part A If a sample containing 2.50 mL of nitroglycerin (density=1.592g/mL) is detonated, how many total moles of gas are produced? Express your answer using three significant figures.
3.70 Detonation of nitroglycerin proceeds as follows: 4C3H,N,09(1)-→ 12CO2(8) 6 N2(a) + O2(8)+ 10H2O(g) (a) If a sample containing 2.00 mL of nitroglycerin (density = 1.592 g/mL) is detonated, how many moles of gas are pro- duced? (b) If each mole of gas occupies 55 L under the condi- tions of the explosion, how many liters of gas are produced? (c) How many grams of N2 are produced in the detonation?
Assume that you have 1.15 g of nitroglycerin in a 579.5 mL steel container at 20.0 ∘C and 1.00 atm pressure. An explosion occurs, raising the temperature of the container and its contents to 425 ∘C. The balanced equation is 4C3H5N3O9(l)→12CO2(g)+10H2O(g)+6N2(g)+O2(g) (Figure 1) Part A How many moles of nitroglycerin were in the container originally? Part B How many moles of gas (air) were in the container originally? Part C How many moles of gas are in the container after...
I need help in these questions: please help ! 1. A balloon containing 157 moles of ammonia gas has an initial volume of 60.0 mL at a temperature of 80.0 C. What is its final temperature when the volume is reduced to 50 mL? 2. An atmospheric sample contains nitrogen at 554 torr, carbon dioxide at 170 torr and oxygen. Assuming STP conditions and a total of 10.0 moles of the gas mixture, what is the partial pressure of oxygen...
Acetylene may be produced from the reaction between calcium carbide and water. How many moles of acetylene are present in a 500.0 mL sample of gas collected over water at 20.0°C and a total pressure of 758 torr? The vapor pressure of water at 20.0 °C is 17.54 mm Hg. 0.0202 moles acetylene 0.0207 moles acetylene 0.297 moles acetylene 0.304 moles acetylene
Assume that you have 1.10 g of nitroglycerin in a 3000 mL steel container at 20.0°C and 1.00 atm pressure. An explosion occurs, raising the temperature of the container and its contents to 425 °C. The balanced equation is 4 CH: N30,(1) + 12 CO2(g) + 10H2O(g) + 6 N2(g) + O2(9) (Figure 1) Part A How many moles of nitroglycerin were in the container originally? 190 AU O ? TICHNO, = Submit Request Answer Part B How many moles...
Under conditions of constant temperature and volume, how many additional moles of gas would have to be added to a flask containing 1.96 moles of gas at 25.0 C and 1.00 atm pressure in order to increase the pressure to 2.3 atm?
A sample of carbon monoxide gas occupies a volume of 263 mL at a pressure of 781.3 torr and a temperature of 399 K. What would its temperature be if the volume were changed to 82 mL at a pressure of 657.5 torr? QUESTION 2 Under conditions of constant temperature and volume, how many additional moles of gas would have to be added to a flask containing 2.7 moles of gas at 25.0 °C and 1.00 atm pressure in order...
•How many N atoms would be present in 0.378 moles of N2O? •2. If you have 4.55 x 1016 NO2 molecules, how many moles would you have? •3. How many grams would you need in order to have 0.885 moles of CuCO3? •4. If you have a 15.0 g sample of PF5, how many PF5 molecules would be in your sample? •5. If you have 3.14 x 1019 FeCl2 molecules, how many milligrams would you have? •6. What is the...
Calculate the number of moles of CO_2 that would be produced if 0.25 g of baking soda completely react with a stoichiometrically equivalent amount of acetic acid. Vinegar is a 5% (w/v) solution of acetic acid (CH_3CO_2H) in water. How many moles of acetic add are contained in 1.00 mL of vinegar? Calculate the number of moles of CO_2 that would be produced if 1.00 mL of vinegar completely reacts with a stoichiometrically equivalent amount of baking soda.