Hi!

I need help with this question:

Sulfur dioxide reacts with chlorine at 227 oC:

SO2(g) +Cl2(g) ↔ SO2Cl2(g)

Kp for this reaction is 5.1 x 10-2 atm-1. Initially, 1.00 g each of SO2 and Cl2 are placed in a 1.00 L reaction vessel. After 15 minutes, the concentration of SO2Cl2 is 45.5 μg/mL. You will determine if the system has reached equilibrium. First, what is Kc (in L/mol)? (A μg is 10-6 g.)
2.093=answer

Next determine all initial concentrations. What is the initial sulfur dioxide concentration (in mol/L or M)?

A=.0156

Determine all concentrations after 15 minutes. What is the chlorine concentration?

A=.0136

What is Q after 15 minutes?
This is the one I can't get. I got 1.49, but that's not right?

Then there's this question which is also an extension:
Calculate the mass (in g) of SO2Cl2 expected at equilibrium.

I got .558 but that's not right either.

Help?

Show your work for (Cl2)

Show your work for Q after 15 min.
Show your work for SO2Cl2 at equil. I obtained about 0.0585 g for SO2Cl2.

thanks! i had already gotten the first couple of answers, which is why i didn't show what i did.

To answer your questions, let's break down the steps and calculations needed.

1. What is Q after 15 minutes?
To determine Q (the reaction quotient) after 15 minutes, we need to calculate the concentrations of each species in the reaction.

Given:
- Initial concentrations: [SO2] = 0.0156 mol/L (or M) and [Cl2] = 0.0156 mol/L (or M)
- Concentration of SO2Cl2 after 15 minutes: [SO2Cl2] = 45.5 μg/mL = 45.5 × 10^-9 g/mL = 45.5 × 10^-9 g / (1 × 10^-3 L) = 4.55 × 10^-5 g/L = 4.55 × 10^-5 × (1 mol / 136.93 g) / (1 × 10^-3 L) = 3.32 × 10^-7 mol/L

Now we can calculate Q using the concentrations:
Q = [SO2Cl2] / ([SO2] * [Cl2])
= (3.32 × 10^-7 mol/L) / ((0.0156 mol/L) * (0.0156 mol/L))
≈ 1.48

Therefore, the value of Q after 15 minutes is approximately 1.48.

2. Calculate the mass of SO2Cl2 expected at equilibrium.
To calculate the mass of SO2Cl2 expected at equilibrium, we need to use the given equilibrium constant (Kp).

Given information:
- Equilibrium constant (Kp) = 5.1 × 10^-2 atm^-1
- Initial pressure of each gas species: [SO2] = [Cl2] = unknown

To find the initial pressure, we can use the Ideal Gas Law:
PV = nRT

Since the volume (V) and temperature (T) are given as 1.00 L and 227 °C (converted to Kelvin: 227 + 273 = 500 K), respectively, and the gas constant (R) is 0.0821 L·atm/(mol·K), we can rearrange the equation to solve for the initial moles (n) of each gas species:
n = PV / RT

Let's calculate the initial moles of SO2:
P = unknown
V = 1.00 L
T = 500 K
R = 0.0821 L·atm/(mol·K)

n(SO2) = (P * V) / (R * T)
= (P * 1.00 L) / (0.0821 L·atm/(mol·K) * 500 K)
= 12.16 * P mol

Similarly, the initial moles of Cl2 will also be 12.16 * P mol.

Now we can substitute the initial moles into the equilibrium expression and solve for the mass of SO2Cl2 at equilibrium:
Kp = (P(SO2Cl2) / (P(SO2) * P(Cl2))
= (mass(SO2Cl2) / (molar mass(SO2Cl2) * P(SO2) * P(Cl2))

Rearranging the equation to solve for the mass of SO2Cl2:
mass(SO2Cl2) = Kp * molar mass(SO2Cl2) * P(SO2) * P(Cl2)

Given:
Kp = 5.1 × 10^-2 atm^-1
molar mass(SO2Cl2) = 136.93 g/mol

We already know the initial pressure of each gas (P(SO2) and P(Cl2)) from the Ideal Gas Law calculation above, which is 12.16 * P.

mass(SO2Cl2) = (5.1 × 10^-2 atm^-1) * (136.93 g/mol) * (12.16 * P) * (12.16 * P)
= 88.98 * P^2 g

Therefore, the expected mass of SO2Cl2 at equilibrium is 88.98 * P^2 grams.

It seems like you may have made a mistake in your calculations for Q and the mass of SO2Cl2. Double-check your work using the formulas and steps provided above to ensure accuracy.