Ammonium nitrate can decompose explosively when heated according to the following equation:
2nh4no3(s) → 2n2(g)+4h2o(g)+o2(g)
how many liters of gas would be formed at 505 ∘c and 1.00 atm pressure from an explosion of 445 g of nh4no3?

354.7 liters of gas are been formed.

Explanation:

A typical problem to apply the Ideal Gases Law.

P.V = n.R.T

Pressure : 1 atm

Volume: Unknown

Mol: 445g/molar weight NH4NO3

R = 0.082 L.atm/mol.K

T°K  = 505°C + 273 =778K

445g/80.04 g/m = 5.56 mol

1 atm . V = 5.56mol . 0.082 L.atm/mol.K . 778K

V= (5.56mol . 0.082 L.atm/mol.K . 778K) /1atm

V= 354,7 L

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.