Calculate the work done when 50.0g of tin dissolves in excess acid at 1.00atm and 25 (degree in celsius)
Sn(s)+2H(aq)----- Sn(aq) +H2(g)
Assume ideal gas behavior
The work done = (pressure)*(increase in volume)
The increase in volume is due to the H2 gas created. 50 g of tin (Sn) is 0.421 moles. That is also the number of moles of H2 that are created. Use tha ideal gas law to compute the added volume due to that gas.
can I get an explanation?
10.27J
Why did the tin get into trouble with the acid? It couldn't keep its cool! But let's do the calculations anyway.
Using the ideal gas law, PV = nRT, we can solve for V to find the increase in volume:
V = (nRT) / P
Where:
n = number of moles of H2 gas (0.421 mol)
R = ideal gas constant (0.0821 L⋅atm/mol⋅K)
T = temperature in Kelvin (25°C = 298 K)
P = pressure (1 atm)
Now, let's plug in the values and calculate the increase in volume. But before we do that, remember to always convert temperature to Kelvin by adding 273 to Celsius temperature.
V = (0.421 mol * 0.0821 L⋅atm/mol⋅K * 298 K) / 1 atm
V ≈ 10.04 L
Now we can calculate the work done:
Work = (pressure) * (increase in volume)
Work = 1 atm * 10.04 L
Work = 10.04 L⋅atm
So, the work done when 50.0 g of tin dissolves in excess acid at 1.00 atm and 25°C is approximately 10.04 L⋅atm. Keep in mind that work is usually expressed in units of joules (J), but since we are given pressure in atm and volume in liters, we'll stick with L⋅atm for now.
To calculate the work done in this scenario, we need to find the increase in volume caused by the formation of hydrogen gas (H2).
First, we determine the number of moles of tin (Sn) that dissolve. We are given that 50.0g of tin dissolves, and the molar mass of tin is approximately 118.71 g/mol. Therefore, the number of moles of tin can be calculated as:
moles of tin (Sn) = mass of tin / molar mass of tin
moles of tin (Sn) = 50.0g / 118.71 g/mol
moles of tin (Sn) ≈ 0.421 mol
Since the balanced chemical equation shows that the stoichiometric ratio between tin and hydrogen gas is 1:2, the number of moles of hydrogen gas produced is also 0.421 mol.
Next, we can use the ideal gas law to determine the volume occupied by the hydrogen gas. The ideal gas law equation is:
PV = nRT
Where:
P is the pressure in atmospheres (1.00 atm in this case),
V is the volume in liters (what we want to find),
n is the number of moles of the gas (0.421 mol),
R is the ideal gas constant (0.0821 L·atm/(mol·K)),
T is the temperature in Kelvin (25 + 273.15 K).
Rearranging the equation to solve for volume (V), we get:
V = (nRT) / P
Substituting the values into the equation:
V = (0.421 mol * 0.0821 L·atm/(mol·K) * (25 + 273.15 K)) / 1.00 atm
Calculating this expression, we find:
V ≈ 9.21 L
Finally, we can calculate the work done using the formula:
Work done = pressure * increase in volume
Work done = 1.00 atm * (9.21 L - 0 L)
Therefore, the work done when 50.0g of tin dissolves in excess acid at 1.00 atm and 25 °C is approximately equal to 9.21 L·atm.