Density= mass/volume
step one :
convert m3 to ml
1m^3 =1000000ml
0.250m^3 x1000000=250000ml
step two: convert mg to g
1mg=0.001g, therefore 4.25 x108mg=0.459g
density is therefore= 0.459g/250000=1.836 x10^-6g/ml
Answer:
At 30 and 2,204
diagonal
liquid phase
2856
top horizontal line
flat
the change from a solid to a liquid
Explanation:
Answer:
We have to fill the acetylene tank with a pressure of 60.67 atm to ensure that you run out of each gas at the same time
Explanation:
Step 1: Data given
Volume of tank 1 = 6.50 L = oxygen
Volume of tank 2 = 4.50 L = acetylene
Pressure in the oxygen tank = 105 atm
Step 2: The balanced equation
2 C2H2 + 5 O2 → 4 CO2 + 2 H2O
For 2 mol C2H2 we need 5 moles O2 to produce 4 moles CO2 and 2 moles H2O
Step 3: Calculate the pressure of the acetylene tank
For 2 mol C2H2 we need 5 moles O2 to produce 4 moles CO2 and 2 moles H2O
This means for each 5 moles O2 we have 2 moles acetylene
Pressure (105 atm) * (2/5) * (6.50 / 4.50) = 60.67 atm
We have to fill the acetylene tank with a pressure of 60.67 atm to ensure that you run out of each gas at the same time
Answer:
-0.85KJ
Explanation:
Given N2(g) + H2(g) <--->2NH3(g)
Kp =[ P(NH3)]²/[P(H2)]³[P(N2)]
Where P is the pressure of the gas
P(H2)b= P(N2) = 125atm
P(NH3) = 200atm
Kp = 2²/(125)³(125)
Kp = 2.048 ×10^-6
∆G = -RTlnKp
R =0.008314 J/Kmol
T = 25 +273/= 298k
= 8.314 ×10^-3 × 298 × ln(2.048 ×10^-6)
= -0.008314 × 298 × (-13.099)
= 32.45KJ
∆G = ∆G° + RTlnKp
∆G = -33.3 + 32.45
∆G = -0.85KJ or -850J
