Answer:
Explanation:
The answer is (4) 4.0 mol. This is a stoichiometry problem. You start with 2.0 mol of C2H6 and obtain the moles of C by multiplying 2.0 by the mole ratio, in this case 2. 2.0*2=4.0mol.
Q = mCΔT
Q is heat, m is mass, C is specific heat, and ΔT is change in temp
First, find how much energy you need to raise the heat to 100C, or the boiling point
Q = (50g)(4.18)(75 degrees) = 15675 J or 15.675 kJ
Then you need 40.7 kJ extra for each mole of water to evaporate it
If you have 50 grams of water and there are 18 grams per mol
50g / 18g = 2.8 moles x 40.7 = 113 kJ extra
15.675 + 113 kJ = 128.7 kJ required
Answer:The acid is strong because it has a calculated K of 7.76x10*
the answer is: protect rights to new products and processes
Answer:
(a) pSO₂Cl₂ = 0.14 atm
pSO₂ = pCl₂ = x = 0.58 atm
(b) Kp = 2.4
Explanation:
Let's consider the following reaction.
SO₂Cl₂(g) ⇄ SO₂(g) + Cl₂(g)
We can calculate the initial pressure of SO₂Cl₂ using the ideal gas equation.
We can find the partial pressures at equilibrium using an ICE chart. In this chart, we complete each row with the pressure or change in pressure in each stage.
SO₂Cl₂(g) ⇄ SO₂(g) + Cl₂(g)
I 0.7201 0 0
C -x +x +x
E 0.7201 - x x x
At equilibrium, the sum of partial pressures is equal to the total pressure.
pSO₂Cl₂ + pSO₂ + pCl₂ = 1.30 atm
(0.7201 - x) + x + x = 1.30 atm
x = 0.58 atm
pSO₂Cl₂ = 0.7201 - x = 0.14 atm
pSO₂ = pCl₂ = x = 0.58 atm
The equilibrium constant (Kp) is: