To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 5.3-L bulb, then filled it with the gas at 1.30atm and 27.0 ∘C and weighed it again. The difference in mass was 7.9g . Identify the gas. Express your answer as a chemical formula.

Please just an answer or an explanation that is easy to understand, like you would a five year old who has big dreams

No that's wrong, it's 28, divide 2, get N2

Well, hello there, little dreamer! Let me explain it to you in a way you'll understand!

So, this researcher had a big ol' bulb, like a balloon, you know? She weighed it when there was nothing inside, and then she put a gas in it and weighed it again. What she found was that the bulb got heavier by 7.9 grams.

Now, the gas she put in there is what we need to figure out. Lucky for us, she told us that the gas is diatomic, which means it's made up of two atoms of the same kind sticking together.

Okay, let's break some things down. The 5.3-L part just tells us how big the bulb is, so we can ignore that for now. The important part is that the gas was at a pressure of 1.30 atm and a temperature of 27.0 degrees Celsius.

Now, using our detective skills (and a little bit of science), we can narrow it down to a few possible gases. One of them is oxygen gas (O2), which is made up of two oxygen atoms sticking together. Another possibility is nitrogen gas (N2), which is made up of two nitrogen atoms sticking together.

But which one is it, you ask? Well, that's the tricky part. We need a little more information to be completely sure. But based on what we know, the most likely answer is oxygen gas (O2).

So, to sum it all up, the gas the researcher put in the bulb is most likely oxygen gas, and we can write it as the chemical formula "O2".

To identify the diatomic gas, we can use the ideal gas law equation, which is:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles of gas
R = ideal gas constant
T = temperature

We can rearrange the equation to solve for the number of moles (n):

n = PV / RT

First, we need to convert the volume from liters to cubic meters. Since 1 liter is equal to 0.001 cubic meters, the volume will be:

V = 5.3 L * 0.001 m³/L = 0.0053 m³

Next, we need to convert the temperature from degrees Celsius to Kelvin. Since the Kelvin scale is shifted by 273.15 units from the Celsius scale, the temperature will be:

T = 27.0 °C + 273.15 = 300.15 K

Now we can substitute the given values into the equation:

n = (1.30 atm) * (0.0053 m³) / (0.0821 L·atm/(mol·K)) * (300.15 K)

Simplifying the equation:

n ≈ 0.002 moles

Since we are dealing with a diatomic gas (X2), the number of moles represents twice the number of molecules. Therefore, the number of molecules is:

2 * 0.002 moles = 0.004 moles

Finally, we can calculate the molar mass of the gas by dividing the difference in mass (7.9 g) by the number of moles (0.004 moles):

Molar mass = 7.9 g / 0.004 moles ≈ 197.5 g/mol

To identify the gas, we look for a diatomic gas with a molar mass close to 197.5 g/mol. In this case, the gas is bromine (Br2), which has a molar mass of approximately 159.8 g/mol. Therefore, the gas in the bulb is not bromine (Br2).

We can try another diatomic gas with a similar molar mass. Chlorine gas (Cl2) has a molar mass of approximately 70.9 g/mol, which is significantly lower than the calculated molar mass. Hence, the gas in the bulb is not chlorine (Cl2) either.

By process of elimination, the gas in the bulb is likely iodine (I2), which has a molar mass of approximately 253.8 g/mol. Therefore, the chemical formula for the gas is iodine (I2).

3.57 moles equals n, so i divide 7.9 by that to get grams per mole, which is 2.2. I divide that by 2 to get Hydrogen, but that's wrong

Thank you. Thank you. A lot

Dream big.

Use PV = nRT
You know P, V, R (0.08206) and T (use T in Kelvin = 273+c).

Solve for n.
Then mols = n = grams/molar mass.
YOu know grams and mols, solve for molar mass and look it up on the periodic table. Post your work if you get stuck but explain what you don't understand.