Answer:
0.27 atm
Explanation:
<em>At 25ºC, Kp = 2.9 x 10⁻³ for the reaction NH₄OCONH₂(s) ⇌ 2 NH₃(g) + CO₂(g). In an experiment carried out at 25ºC, a certain amount of NH₄OCONH₂ is placed in an evacuated rigid container and allowed to come to equilibrium. Calculate the total pressure in the container at equilibrium.</em>
Step 1: Make an ICE chart
Solid and liquids are ignored in ICE charts.
NH₄OCONH₂(s) ⇌ 2 NH₃(g) + CO₂(g)
I 0 0
C +2x +x
E 2x x
Step 2: Write the pressure equilibrium constant expression (Kp)
Kp = [NH₃]² × [CO₂]
Kp = (2x)² × x
2.9 × 10⁻³ = 4 x³
x = 0.090 atm
Step 3: Calculate the pressures at equilbrium
pNH₃ = 2x = 2(0.090 atm) = 0.18 atm
pCO₂ = x = 0.090 atm
The total pressure is:
P = 0.18 atm + 0.090 atm = 0.27 atm
Answer:
METAL: found in periodic table, lithium, shiny, lose electrons easily, good conductor, elements
NONMETAL: brittle, ductile, semimetals, found in periodic table, often gain electrons, semiconductors, carbon, shiny, poor conductor, elements
METALLOID: solid, non- ductile, malleable, found in periodic table, silicon, shiny, can be liquids, elements
Answer:
1.evaperation
2.condenstation
3.precipatation
Explanation:
So I guess condenstation leads to precipatation-
Answer:
The net ionic equation shows the actual reaction more clearly and closer to reality because it writes soluble ionic compounds as the ions and then cancel the spectator ions not involved in the chemical reaction . The net ionic equation results shows the actual chemical reaction taking place.
Answer:
2NaOH + CO2 -> Na2CO3 + H2O
1) Find the moles of each substance
2) Determine the limitting reagent
∴ Carbon dioxide is limitting as it has a smaller value.
3) multiply the limiting reagent by the mole ratio of unknown over known
n(H2O ) = 0.3976369007 × 1/2
= 0.1988184504 moles
4) Multiply the number of moles by the molar mass of the substance.
m = 0.1988184504 × (1.008 × 2 + 16.00)
= 0.1988184504 × 18.016
= 3.581913202 g
Explanation:
