A) B) c) d) E) Be sure to answer all parts. When ammonium nitrite (NH4N02) is he

Question

A)

B)

c)

d)

E)

Be sure to answer all parts. When ammonium nitrite (NH4N02) is heated, it decomposes to liquid water and nitrogen gas. This property is used to inflate some tennis balls. Write a balanced equation for the reaction. Include phase symbols. (Click in the answer box to activate the palette. ) Calculate the quantity (in grams) of NH4N02 needed to inflate a tennis ball to a volume of 73. 00 mLat 1. 33 atm and 22 Degree C. Enter your answer in the provided box. Some commercial drain cleaners contain a mixture of sodium hydroxide and aluminum powder. When the mixture is poured down a clogged drain, the following reaction occurs: The heat generated in this reaction helps melt away obstructions such as grease, and the hydrogen gas released stirs up the solids clogging the drain. Calculate the volume of I| formed at 28. 5 degree C and 1. 00 atm if 4. 15 g of A1 is treated with an excess of NaOH. Be sure to answer all parts. Propane (C3 H8) burns in oxygen to produce carbon dioxide gas and water vapor. (a) Write a balanced equation for this reaction. Include all reaction states. Calculate the number of liters of carbon dioxide measured at STP that could be produced from 8. 00 g of propane. Be sure to answer all parts. A mixture of methane (CH4) and ethane (C2H6) is stored in a container at 294 mm Hg. The gases arc burned in air to form CO2 and H2O. If the pressure of CO2 is 347 mm Hg measured at the same temperature and volume as the original mixture, calculate the mole fraction of the gases. Mole fraction of methane: Mole fraction of ethane: Enter your answer in the provided box. Calculate the volume (in liters) occupied by 1. 51 moles of nitric oxide (NO) at 6. 22 atm and 71 Degree C.

Explanation / Answer

A.

(a)

NH4NO2(s)> N2(g) + 2H2O(l)

(b)

PV = nRT

n = 1.33*0.073/0.0821*295 = 4.009*10^-3

moles of N2 required = 4.009*10^-3

moles of NH4NO2 required = 4.009*10^-3

mass of NH4NO2 = 2.56576 gram

B.

mass of aluminium = 4.15 gram

moles of A = 83/540

moles of H2 produced = (3/2)*(83/540) = 83/360

volume of H2 = (83/360)*0.0821*301.5/1 = 5.707 L

C.

C3H8(g) + 5O2(g) --------------> 3CO2(g) + 4H2O(g)

mass of propane = 8 gram

moles of propane = 8/44 = 2/11

moles of CO2 produced = (2/11)*3 = 6/11

volume of CO2 = (6/11)*0.0821*273/1 = 12.225 L

D.

let partial pressure of methane = x

partial pressure of ethane = 294 - x

after burning

partail pressure of CO2 due to methane = x

partial pressure of CO2 due to ethane = 2(294 - x)

tatal pressure of CO2 = 347 = x + 2(294 - x) = 588 - x

=> x = 241

mole fraction = partial pressure/total pressur

mole fraction of CH4 = 241/294 = 0.8197

mole fraction of C2H6 = 0.1803

E.

volume = 1.51*0.0821*344/6.22 = 6.856 L

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