Answer:
1.77 atm
Explanation:
We have to check the <u>values that gives the problem</u>:
V= 70 L
mass =354.5 g
Molas weight= 70.9 g/mol
T=30 ºC
P= ?
We can find the <u>moles of chlorine</u> if we use the<u> molar weight</u>:
Now, we have the moles, volume, temperature therefore we can use the <u>ideal gas equation</u>:
We know the <u>R value</u>:
We have <u>“K” units for the temperature</u>, so we need to do the <u>conversion</u>:
With all the data we can plug the values into the equation:
I hope it helps!
Answer:
53.7kJ/mol
Explanation:
Using Arrhenius equation
Given
T1 = 12°C = 273 + 12 = 285K
T2 = 21°C = 273 + 21 = 294K
k = A exp(-Ea/RT)
Where k = Rate constant
A = the pre-exponential factor
Ea = the activation energy
R = the Universal Gas Constant = 8.314J/kmol
T = the temperature
Taking logarithms of both sides of the Arrhenius Equation.
ln(k) = ln(A) - Ea/RT
If there are the rates at two different temperatures, we can derive the expression to be;
ln(k2/k1) = Ea/R(1/T1 - 1/T2)
The reaction doubles the rate constant
So, k2/k1 = 2 (Given)
Then we have
ln(2) = Ea/8.314(1/285 - 1/294)
ln(2) * 8.314 = Ea*(1/285 - 1/294)
6.9314E-1 * 8.314 = Ea*(1/285 - 1/294)
5.7628 = Ea*(1/285 - 1/294)
5.7628 = Ea*1.0741E-4
Ea = 5.7628 / 1.074E-4
Ea = 53657.35567970204J
Ea = 53.7kJ/mol
40 grams ÷ 40.08 grams/moles = 1 mole
Answer:
Re=309926.13
Explanation:
density=92.8lbm/ft3*(0.45kg/1lbm)*(1ft3/0.028m3)=1491.43kg/m3
viscosity=4.1cP*((1*10-3kg/m*s)/1cP)=0.0041kg/m*s
velocity=237ft/min*(1min/60s)*(0.3048m/1ft)=1.2m/s
diameter=28inch*(0.0254m/1inch)=0.71m
Re=(density*velocity*diameter)/viscosity=(1491.43kg/m3*1.2m/s*0.71m)/0.0041kg/m*s
Re=309926.13
