A 8.80-g sample of solid SnCl2·2H2O was heated such that the water turned to steam and was driven off. Assuming ideal behavior, what volume would that steam occupy at 1.00 atm and 100.0 °C?
A or himesh or whatever,
Why not work this the same way as steam out of AlCl3.62O
doesnt work the same way as ALCL3.6H2O
To calculate the volume of steam produced, we need to use the ideal gas law equation:
PV = nRT
where:
P = pressure (1.00 atm)
V = volume (unknown)
n = number of moles of steam
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (100.0 °C + 273.15 = 373.15 K)
First, let's calculate the number of moles of steam produced from the given mass of water:
1. Calculate the molar mass of SnCl2·2H2O:
Molar mass of Sn = 118.71 g/mol
Molar mass of Cl2 = 70.90 g/mol
Molar mass of H2O = 18.02 g/mol
Total molar mass = (118.71) + (2 * 70.90) + (2 * 18.02) = 254.55 g/mol
2. Calculate the number of moles of SnCl2·2H2O:
moles = mass (g) / molar mass (g/mol)
moles = 8.80 g / 254.55 g/mol ≈ 0.0345 mol
Since SnCl2·2H2O has 2 moles of water (H2O), the number of moles of steam produced is twice the number of moles of SnCl2·2H2O:
moles of steam = 2 * 0.0345 mol = 0.069 mol
Now, we can substitute the values into the ideal gas law equation to solve for the volume (V):
PV = nRT
V = (nRT) / P
V = (0.069 mol * 0.0821 L·atm/mol·K * 373.15 K) / (1.00 atm)
V ≈ 1.97 L
Therefore, the steam would occupy approximately 1.97 liters at 1.00 atm and 100.0 °C.
To find the volume of the steam, we need to use the Ideal Gas Law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.
First, we need to calculate the number of moles of water vapor produced during the heating process. We can do this by using the molar mass of water, which is 18.015 g/mol.
Given that the sample initially had a mass of 8.80 g and SnCl2·2H2O has a molar mass of 225.63 g/mol, we can calculate the number of moles of SnCl2·2H2O:
moles of SnCl2·2H2O = mass / molar mass
moles of SnCl2·2H2O = 8.80 g / 225.63 g/mol
Next, we need to calculate the number of moles of water in the SnCl2·2H2O formula. Since there are two moles of water per mole of SnCl2·2H2O, we multiply the number of moles of SnCl2·2H2O by 2:
moles of water = 2 * moles of SnCl2·2H2O
Now, we know the number of moles of water vapor produced.
To find the volume, we can rearrange the Ideal Gas Law equation to solve for V:
V = (nRT) / P
Plug in the known values:
V = (moles of water * R * T) / P
Given that R (the gas constant) is 0.0821 L·atm/(mol·K), the temperature T is 100.0 °C converted to Kelvin (373.15 K), and the pressure P is 1.00 atm, we can solve for V.
V = (moles of water * 0.0821 L·atm/(mol·K) * 373.15 K) / 1.00 atm
Now, substitute the value obtained for moles of water into the equation to calculate the volume of the steam.