Answer:
14.048 moles I believe.
Explanation:
(8.46 * 10^24) / ( 6.022 * 10^23) = 14.048
From ideal gas equation that is PV=nRT
n(number of moles)=PV/RT
P=760 torr
V=4.50L
R(gas constant =62.363667torr/l/mol
T=273 +273=298k
n is therefore (760torr x4.50L) /62.36367 torr/L/mol x298k =0.184moles
the molar mass of NO2 is 46 therefore density= 0.184 x 46=8.464g/l
Answer: Mass Of CFC that needs to evaporate for the freezing of water = 328.24 g
Explanation: Heat gained by the CFC = Heat lost by water
Heat lost by water = Heat required to take water's temperature to 0°c + Heat required to freeze water at 0°c
Heat required to take water's temperature from 33°c to 0°c = mCΔT
m = 201g, C = 4.18 J/(gK), ΔT = 33
mCΔT = 201 × 4.18 × 33 = 27725.94 J
Heat required to freeze water at 0°c = mL
m = 201g, L = 334 J/g
mL = 201 × 334 = 67134 J
Heat gained by CFC to vaporize = mH = 27725.94 + 67134 = 94859.94 J
H = 289 J/g, m = ?
m × 289 = 94859.9
m = 328.24 g
QED!!
According to the ideal gas law, partial pressure is inversely proportional to volume. It is also directly proportional to moles and temperature. At equilibrium in the following reaction at room temperature, the partial pressures of the gases are found to be PN2 = 0.094 atm, PH2 = 0.039 atm, and PNH3 = 0.003 atm.
<h3>Equilibrium partial pressures</h3>
The initial partial pressures of CO and water are 4.0 bar and 4.0 bar respectively.
The equilibrium partial pressures (in the bar) of CO, H2O, CO2, and H2 are 4−p,4−p, and respectively.
Let p bar be the equilibrium partial pressure of hydrogen.
The expression for the equilibrium constant is
Kp=PCOPH2OPCO2PH2=(4−p)(4−p)p×p=0.1
p=1.264−0.316p
p=0.96 bar.
To learn more about equilibrium constant visit the link
brainly.com/question/10038290
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Answer:
Br
Explanation:
atomic size grows as we go from left to right side of the periodic table since Si has atomic number of 14 and Br 35,we can say Br has more atomic size.
