A sealed flask contains 1 mole of hydrogen and 3 moles of helium gas at 20DC. If the total pressure is 40kPa, what is the partial pressure of the Hydrogen gas?
AND :)
The data below was obtained by a student in order to determine the percent of water in a Hydrate:
Mass of the Hydrate..............5.0gram
Mass of the Anhydrous Compound.. 3.2gram
What is the percent in the Hydrate?
PLEASE ANSWER THESE ASAP :D
Use Raoult's Law
Pa=XaPt
where Xa is the mole fraction (1/4) and Pt is the total pressure which is 40.
So (1/4)40=10kPa
To calculate the partial pressure of hydrogen gas in the sealed flask, we can use the ideal gas law, which states:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
In this case, we are given the total pressure (P = 40 kPa), the number of moles of hydrogen (n = 1 mole), the number of moles of helium (n = 3 moles), and the temperature (T = 20°C = 293.15 K).
To find the partial pressure of hydrogen, we need to subtract the pressure contributed by the helium gas from the total pressure. The moles of helium (n = 3 moles) can be used to calculate its pressure.
Let's go step by step:
Step 1: Convert temperature to Kelvin
T = 20°C + 273.15 = 293.15 K
Step 2: Calculate the pressure contributed by helium.
From the ideal gas law, we have:
PV = nRT
Thus, P = nRT / V
Using the given values:
P_helium = (3 moles) * (8.314 J/(mol·K)) * (293.15 K) / V
Step 3: Calculate the partial pressure of hydrogen.
The total pressure (P_total) is 40 kPa, and we want to find the partial pressure of hydrogen (P_hydrogen). Since the total pressure is the sum of the partial pressures of each gas, we have:
P_total = P_hydrogen + P_helium
Rearranging the equation:
P_hydrogen = P_total - P_helium
Substituting the values:
P_hydrogen = (40 kPa) - P_helium
Since we don't have the volume (V), we cannot calculate the exact partial pressure.
Moving on to your second question:
To find the percent of water in the hydrate, we need to determine the mass of water and the mass of the anhydrous compound.
Let's go step by step:
Step 1: Determine the mass of water.
Mass of water = Mass of hydrate - Mass of anhydrous compound
Mass of water = 5.0 g - 3.2 g
Mass of water = 1.8 g
Step 2: Calculate the percent of water in the hydrate.
Percent of water = (Mass of water / Mass of hydrate) * 100
Percent of water = (1.8 g / 5.0 g) * 100
Percent of water = 36%
Hence, the percent of water in the hydrate is 36%.
Sure! I'd be happy to help answer your questions.
1. Partial Pressure of Hydrogen Gas:
To find the partial pressure of the hydrogen gas, we need to use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the amount of gas in moles, R is the ideal gas constant, and T is the temperature in Kelvin.
Given that the total pressure (P) is 40 kPa, the number of moles of hydrogen (n) is 1 mole, the number of moles of helium is 3 moles, and the temperature (T) is 20 degrees Celsius, we need to convert the temperature to Kelvin.
To convert Celsius to Kelvin, we use the formula: T(K) = T(°C) + 273.15.
So, 20°C + 273.15 = 293.15 K.
Now we can plug these values into the ideal gas law equation: PV = nRT.
For the hydrogen gas:
P(H2) * V = n(H2) * R * T.
Since the volume (V) is constant (as it is a sealed flask), we can ignore it.
Therefore, P(H2) = n(H2) * R * T / V.
Using the values we have:
n(H2) = 1 mole
R = 8.314 J/(mol·K) (ideal gas constant)
T = 293.15 K
Now we can calculate the partial pressure of hydrogen gas:
P(H2) = 1 mole * 8.314 J/(mol·K) * 293.15 K / V.
Please provide the value of V (volume) to calculate the partial pressure accurately. Remember to convert the units to match the value provided.
2. Percent of Water in a Hydrate:
To find the percent of water in a hydrate, we need to determine the mass of water and the mass of the anhydrous compound.
Given:
Mass of the Hydrate = 5.0 grams
Mass of the Anhydrous Compound = 3.2 grams.
To calculate the percent of water in the hydrate, we use the following formula:
Percent of Water = (Mass of Water / Mass of Hydrate) * 100.
Substituting the given values:
Percent of Water = (Mass of Water / 5.0 grams) * 100.
To determine the mass of water, we subtract the mass of the anhydrous compound from the total mass of the hydrate:
Mass of Water = Mass of Hydrate - Mass of Anhydrous Compound.
Substituting the given values:
Mass of Water = 5.0 grams - 3.2 grams.
Now we can calculate the percent of water in the hydrate:
Percent of Water = ((5.0 grams - 3.2 grams) / 5.0 grams) * 100.
Simplifying the calculation will give you the final answer.