A 2.00g sample of a gas SX6 has a volume of 329.5 cm3 at 1.00 atm and 20 celcius. What element is X?
Note the correct spelling of celsius.
Use PV = nRT
solve for n.
use moles = g/molar mass to find the molar mass of SX6, subtract the atomic mass of S to find the mass of 6 X atoms. Of course you can finish.
To determine the element X in the gas SX6, we can use the molar mass and ideal gas equation.
1. Start by converting the given volume from cm3 to liters:
329.5 cm3 = 329.5 cm3 * (1 L / 1000 cm3) = 0.3295 L
2. Next, use the ideal gas equation, PV = nRT, to find the moles of gas:
P = pressure (1.00 atm)
V = volume (0.3295 L)
n = moles of gas
R = ideal gas constant (0.0821 L•atm/mol•K)
T = temperature in Kelvin
Since the gas is at 20 degrees Celsius, we need to convert it to Kelvin:
T(K) = T(°C) + 273.15 = 20 + 273.15 = 293.15 K
Rearrange the ideal gas equation to solve for moles:
n = PV / RT = (1.00 atm * 0.3295 L) / (0.0821 L•atm/mol•K * 293.15 K)
n = 0.00401777 mol
3. Next, calculate the molar mass of the gas SX6 by dividing the sample's mass (2.00g) by the moles of gas:
Molar mass (g/mol) = mass (g) / moles of gas
Molar mass (g/mol) = 2.00 g / 0.00401777 mol
Molar mass (g/mol) = 497.8 g/mol
4. Finally, use the periodic table to find an element with a molar mass close to 497.8 g/mol. Comparing the molar mass, we can see that the element X in the gas SX6 is Selenium (Se) with a molar mass of 78.971 g/mol.
Therefore, the element X in the gas SX6 is Selenium.
To determine the element X in gas SX6, 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 of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
First, let's convert the given temperature from Celsius to Kelvin. The conversion formula is: K = °C + 273.15.
So, T = 20°C + 273.15 = 293.15 K.
Next, we rearrange the ideal gas law equation to solve for n (the number of moles of gas): n = PV / RT.
We are given:
- P = 1.00 atm (pressure),
- V = 329.5 cm3 (volume), and
- T = 293.15 K (temperature).
However, we still need the value of R, the ideal gas constant. The value of R depends on the units used for pressure and volume. In this case, the given pressure is in atm, and the given volume is in cm3.
The ideal gas constant in these units is R = 0.0821 L·atm/(K·mol).
Converting the given volume from cm3 to liters:
V = 329.5 cm3 = 329.5/1000 L = 0.3295 L.
Now, we can substitute all the values into the equation: n = (1.00 atm) * (0.3295 L) / (0.0821 L·atm/(K·mol)) * (293.15 K).
By cancelling units and performing the calculation, we find the value of n in moles.
Finally, based on the molecular formula SX6, we can divide the obtained number of moles by the mass of the sample to find the molar mass.
Molar mass = mass of sample / moles of gas.
So, molar mass = 2.00 g / n (moles of gas).
Dividing the molar mass by 6 (because there are six X atoms in SX6), we can find the molar mass of element X.
Once we have the molar mass of X, we can compare it to the molar masses of known elements to identify the element X that fits the given molar mass value.