What volume (mL) of sulfur dioxide can be produced by the complete reaction of 3.82 g of calcium sulfite with excess HCl, when the final SO2 pressure is 827 torr at 44 degrees celsius?

To calculate the volume of sulfur dioxide produced, we can use the ideal gas law:

PV = nRT

Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)

First, let's convert the given pressure from torr to atm:
1 atm = 760 torr

So, the final pressure in atm is:
827 torr / 760 torr/atm = 1.088 atm

Next, let's convert the given temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15

So, the temperature in Kelvin is:
44°C + 273.15 = 317.15 K

Now, let's calculate the number of moles of sulfur dioxide:
Using the balanced chemical equation:
CaSO3 + 2HCl → CaCl2 + H2O + SO2

The molar mass of calcium sulfite (CaSO3) is:
Ca: 1 mol x 40.08 g/mol = 40.08 g/mol
S: 1 mol x 32.07 g/mol = 32.07 g/mol
O: 3 mol x 16.00 g/mol = 48.00 g/mol

Total molar mass = 40.08 g/mol + 32.07 g/mol + 48.00 g/mol = 120.15 g/mol

Now, let's calculate the number of moles using the given mass of calcium sulfite:
moles = mass / molar mass
moles = 3.82 g / 120.15 g/mol = 0.03182 mol

Since the reaction is 1:1 between calcium sulfite and SO2, the number of moles of sulfur dioxide will also be 0.03182 mol.

Now, let's calculate the volume using the ideal gas law:
PV = nRT

V = (nRT) / P
V = (0.03182 mol)(0.0821 L·atm/(mol·K))(317.15 K) / 1.088 atm

V ≈ 0.788 L

Finally, let's convert the volume from liters to milliliters:
1 L = 1000 mL

So, the volume of sulfur dioxide produced is:
0.788 L x 1000 mL/L = 788 mL

Therefore, the volume of sulfur dioxide produced is approximately 788 mL.

To solve this problem, we need to use the ideal gas law equation:

PV = nRT,

where:
P is the pressure (in atm),
V is the volume (in liters),
n is the number of moles,
R is the ideal gas constant (0.0821 L·atm/(K·mol)), and
T is the temperature (in Kelvin).

We'll start by converting the given pressure from torr to atm:

1 torr = 1/760 atm

827 torr * (1/760 atm/torr) = 1.087 atm

Next, we need to convert the given temperature from Celsius to Kelvin:

44 degrees Celsius + 273.15 = 317.15 K

Now, we need to calculate the number of moles of sulfur dioxide (SO2) using the given mass of calcium sulfite (CaSO3).

First, determine the molar mass of CaSO3:
Ca: 40.08 g/mol
S: 32.06 g/mol
O (3 atoms): 3 * 16.00 g/mol = 48.00 g/mol

Total molar mass = 40.08 g/mol + 32.06 g/mol + 48.00 g/mol = 120.14 g/mol

Now, use the molar mass to calculate the number of moles:
3.82 g CaSO3 * (1 mol CaSO3/120.14 g) = 0.0318 mol CaSO3

Since the reaction is balanced, each mole of CaSO3 will produce one mole of SO2.

Therefore, the number of moles of SO2 is also 0.0318 mol.

Now, we can rearrange the ideal gas law equation to solve for volume (V):

V = nRT/P

Plugging in the values we've calculated:

V = (0.0318 mol * 0.0821 L·atm/(K·mol) * 317.15 K) / 1.087 atm
V ≈ 0.746 L

Finally, we convert the volume from liters to milliliters:

0.746 L * (1000 mL/L) = 746 mL

Therefore, the volume of sulfur dioxide produced is approximately 746 mL.

1. Write the balanced equation.

2. Convert 3.82 g CaSO3 to moles. #moles = grams/molar mass.
3. Using the coefficients in the balanced equation, convert moles CaSO3 to moles SO2.
4. Use PV = nRT to convert moles SO2 to volume (in liters) then convert L to mL. Don't forget T is in Kelvin.
Post your work if you get stuck.