hen how do u find:
the volume of the H2O released, measured at 220 degrees C and 735mm Hg?
The inital volume is 0.337 grams
I can't make head or tails of the question as it is posted.
Perhaps you want to know the volume of 0.337 g H2O at the P and T of the problem. If so just substitute into PV = nRT
P = 735/760 = ?
T = 220 + 273 = ? K
V = solve for this
n = 0.337/18 = ?
R = 0.08206
Post your work if you stuck.
To find the volume of water released, measured at 220 degrees Celsius and 735 mmHg, given the initial volume of 0.337 grams, we can use the ideal gas law equation.
1. Convert the mass of water (0.337 grams) to moles using its molar mass. The molar mass of water (H2O) is approximately 18.01528 g/mol.
molar mass of H2O = 2(atomic mass of hydrogen) + atomic mass of oxygen = 2(1.00784 g/mol) + 15.999 g/mol ≈ 18.01528 g/mol
moles of H2O = 0.337 grams / 18.01528 g/mol
2. Use the ideal gas law equation, PV = nRT, to find the volume of water released. Rearrange the equation to solve for volume (V):
V = (nRT) / P
Where:
- V is the volume in liters
- n is the number of moles
- R is the ideal gas constant (0.0821 L·atm/(mol·K))
- T is the temperature in Kelvin (220 degrees Celsius + 273.15 = 493.15 K)
- P is the pressure in atm (735 mmHg / 760 mmHg/atm)
V = (moles of H2O * R * T) / P
3. Plug in the values into the equation and calculate:
V = (moles of H2O * 0.0821 L·atm/(mol·K) * 493.15 K) / (735 mmHg / 760 mmHg/atm)
Remember to use the appropriate unit conversions as indicated.
4. Calculate using the given mass:
moles of H2O = 0.337 g / 18.01528 g/mol ≈ 0.01870 mol
V = (0.01870 mol * 0.0821 L·atm/(mol·K) * 493.15 K) / (735 mmHg / 760 mmHg/atm)
5. Calculate the final volume:
V ≈ 0.099 L or 99 mL
Therefore, the volume of water released, measured at 220 degrees Celsius and 735 mmHg, is approximately 0.099 liters or 99 milliliters.
To find the volume of H2O released, measured at 220 degrees C and 735 mm Hg, you need to use the ideal gas law equation: PV = nRT. Here's how to calculate it step by step:
Step 1: Convert the initial mass of H2O to moles.
To convert grams to moles, you need to divide the mass by the molar mass of H2O. The molar mass of water (H2O) is approximately 18.015 g/mol. Let's assume the molar mass is exact. Thus, the number of moles can be calculated as follows:
moles = mass / molar mass
moles = 0.337 g / 18.015 g/mol
Step 2: Calculate the molar volume of H2O at the given temperature and pressure.
To calculate the molar volume, we need to use the ideal gas law equation. However, we need to rearrange the equation to solve for volume (V).
PV = nRT
V = (nRT) / P
Where:
V = volume (in liters)
n = moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
P = pressure (in atm)
But first, let's convert the temperature from degrees Celsius to Kelvin:
T(K) = T(C) + 273.15
T(K) = 220°C + 273.15 = 493.15 K
Now, we can calculate the molar volume:
V = (nRT) / P
V = (moles × R × T) / P
V = (0.337 mol × 0.0821 L·atm/(mol·K) × 493.15 K) / 735 mmHg
Step 3: Convert the volume to the desired units.
To convert the volume from liters to a different unit, you can use conversion factors. For example, if you want to convert it to milliliters (mL), you can use the conversion factor: 1 liter = 1000 milliliters.
V(ml) = V(L) × 1000 mL/L
By substituting the calculated V in liters into the formula above, you will get the volume of H2O released in milliliters.
Note: Remember to always perform unit conversions to ensure consistency throughout the calculation.
That's it! By following these steps, you should be able to find the volume of H2O released, measured at 220 degrees C and 735 mmHg, given an initial volume of 0.337 grams.