1.Calculate the density of oxygen, O2, under each of the following conditions:

STP
1.00 atm and 20.0 ∘C

2.To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 4.3-L bulb, then filled it with the gas at 1.90atm and 20.0 ∘C and weighed it again. The difference in mass was 9.5g . Identify the gas.

3.If 2.9g of N2 gas has a volume of 0.50L and a pressure of 6.8atm , what is its Kelvin temperature?

At STP is is 32/22.4 = ?

At 1 atm and 20C use PMolar mass = density*RT
and solve for density. Remember T must be in kelvin.
Use P*molar mass = gRT/V
Solve for molar mass and since it is X2 divide by 2 to find atomic mass. Look it up on the periodic table.

1. To calculate the density of oxygen at standard temperature and pressure (STP), you need to know the molar mass of oxygen and the molar volume at STP.

1 mole of gas at STP has a volume of 22.4 liters. The molar mass of oxygen (O2) is approximately 32 g/mol.

The density (D) of a gas is calculated using the formula:
D = (molar mass) / (molar volume)

At STP, the molar volume is 22.4 liters/mol. Therefore, the density of oxygen at STP would be:
D = 32 g/mol / 22.4 liters/mol

2. To identify the gas in the bulb, we can use the ideal gas law equation which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L*atm/(mol*K)), and T is the temperature in Kelvin.

In the experiment, the researcher measured the change in mass of the bulb after filling it with the gas. This difference in mass represents the mass of the gas itself.

Using the ideal gas law, we can rearrange it to solve for the number of moles of gas (n):
n = (PV) / (RT)

Given:
P = 1.90 atm
V = 4.3 L
T = 20.0 °C = 20.0 + 273.15 K

Calculate:
n = (1.90 atm * 4.3 L) / (0.0821 L*atm/(mol*K) * (20.0 + 273.15 K)

Use the calculated value of n to determine the molar mass of the gas. Divide the difference in mass (9.5 g) by the number of moles (n) to find the molar mass.

Compare the molar mass to the molar masses of known diatomic gases to identify the gas.

3. To find the Kelvin temperature, we can use the ideal gas law equation.

Given:
m = 2.9 g
V = 0.50 L
P = 6.8 atm
R = 0.0821 L*atm/(mol*K)

First, calculate the number of moles (n):
n = m / molar mass

Next, rearrange the ideal gas law equation to solve for temperature (T):
T = (P * V) / (n * R)

Substitute the given values into the equation to find the Kelvin temperature.

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