Question

What is the rms speed of Cl2 molecules at 335 K?

Answer 1

That's sqrt(3RT/M)

R is 8.314
T is 335 K
M is molar mass Cl2.
Substitute and solve.

Answer 2

[AI-generated answer — Step-by-Step Bot]

To find the root mean square (rms) speed of Cl2 molecules at a given temperature, you can use the following equation:

v(rms) = sqrt((3RT) / (M))

Where:
v(rms) is the root mean square speed,
R is the ideal gas constant (8.314 J/(mol·K) or 0.0821 L·atm/(mol·K)),
T is the temperature in Kelvin,
M is the molar mass of Cl2.

For Cl2, the molar mass (M) is 70.906 g/mol.

Let's substitute these values into the equation:

v(rms) = sqrt((3 * 0.0821 * 335) / 70.906)

Calculating this expression gives us:

v(rms) ≈ sqrt(0.38344) ≈ 0.62 km/s

Therefore, the rms speed of Cl2 molecules at 335 K is approximately 0.62 km/s.

Answer 3

[AI-generated answer — Explain Bot]

To find the root-mean-square (rms) speed of Cl2 molecules at 335 K, you can use the following equation:

v(rms) = √(3 * k * T / m)

Where:
v(rms) is the rms speed
k is the Boltzmann constant (1.38 x 10^-23 J/K)
T is the temperature in Kelvin
m is the molar mass of Cl2 (70.91 g/mol)

First, convert the temperature from Celsius to Kelvin:
335 K = 335 + 273.15 = 608.15 K

Next, plug the values into the equation:

v(rms) = √(3 * 1.38 x 10^-23 J/K * 608.15 K / 70.91 g/mol)

Now, simplify and calculate the rms speed:

v(rms) = √(2.05 x 10^-20 J/ g)

Note: The molar mass of Cl2 is 70.91 g/mol, so the units of J/mol cancel out, leaving us with J/g.

To calculate the square root, you can use a scientific calculator or the square root function on your computer or mobile device.

Once you calculate the square root, you will have the rms speed of Cl2 molecules at 335 K.