What is the total volume of gases produced at 1365 K and 1.000 atm pressure when

Question

What is the total volume of gases produced at 1365 K and 1.000 atm pressure when 192 g of ammonium nitrate undergoes the following decomposition reaction? In which of the following reactions will the pressure increases upon completion of the reaction at constant temperature? Sodium azide decomposes rapidly to produce nitrogen gas. What mass of sodium azide will inflate a 60.0 L airbag for car to a pressure of 1.50 atm at 32 degree C? A particular gas exerts a pressure of 4.98 Times 10^4 Pa. What is this pressure in units of atmospheres? The pressure of O_2 in a 15.0 L flask is 322 mm Hg at 44 degree C. What mass of O_2 is in the flast?

Explanation / Answer

29)

we know that

moles = mass / molar mass

so

moles of NH4N02 = 192 / 64 = 3

now

NH4N02 --> N2 (g) + 2 H20 (g)

moles of gases = 3 x moles of NH4N02 reacted

moles of gaeses = 3 x 3 = 9

now

PV = nRT

1 x V = 9 x 0.0821 x 1365

V = 1010

V = 1.01 x 10^3 L

answer is e) 1.01 x 10^4 L

31)

for the pressure to increase

more amount of gases should be formed

so

d) 4 NH3 (g) + 5 02 (g) ---> 4 N0 (g) + 6 H20 (g)

33)

we know that

PV = nRT

for N2

1.5 x 60 = n x 0.0821 x 305

n = 3.6

so

moles of N2 required = 3.6

now

2 NaN3 --> 2 Na + 3 N2

moles of NaN3 required = ( 2/3) x moles of N2

moles of NaN3 = ( 2/3) x 3.6 = 2.4

now

mass = moles x molar mass

so

mass of NaN3 = 2.4 x 65 = 156

so

answer is c) 156 g

35) we know that

1 atm = 101.3 x 1000 Pa

so

pressure = 4.98 x 10^4 Pa

= 4.98 x 10^4 / 101.3 x 1000 atm

= 0.491 atm

so the answer is option a) 0.491 atm

36)

PV = nRT

( 332/760) x 15 = n x 0.0821 x 317

n = 0.25177

now

mass = 0.25177 x 32

mass = 8.06

so

mass of 02 is 8.06 g

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