A gas mixture is made by combining 5.7 g each of Ar , Ne , and an unknown diatomic gas. At STP, the mixture occupies a volume of 12.88 L. What is the molar mass of the unknown gas?

The molar mass of unknown diatomic gas is 38 grams

Explanation:

At STP:

The temperature and pressure conditions are 273 K and 1 atm respectively.

To calculate the number of moles, we use the equation given by ideal gas equation:

PV = nRT

P = Pressure of the gas  = 1.00 atm

V = Volume of the gas = 12.88 L

n = number of moles of mixture = ?

R = Gas constant =

T = Temperature of the gas

Putting values in above equation, we get:

To calculate the number of moles, we use the equation:

    .....(1)

Given mass of argon = 5.7 g

Molar mass of argon = 39.95 g/mol

Putting values in equation 1, we get:

Given mass of neon = 5.7 g

Molar mass of neon = 20.2 g/mol

Putting values in equation 1, we get:

Moles of unknown diatomic gas = [0.575 - (0.143 + 0.282)] = 0.150

Now, calculating the molar mass of unknown diatomic gas from equation 1, we get:

Given mass of unknown diatomic gas = 5.7 g

Moles of unknown diatomic gas = 0.150 moles

Putting values in equation 1, we get:

Hence, the molar mass of unknown diatomic gas is 38 grams

it forms an anion that has a larger radius. anions have a negative charge and are larger than the original atom.

(newtons first law)

conservation of momentum law states :

momentum before collision = momentum after collision

momentum p (kg-m/s)= mass * velocity

say moving car=1 000 kg, velocity = 10 m/s then p = 1 000*10= 10 000 kg-m/s

say still car = 2 000 kg, velocity = 0 m/s then p = 2 000* 0 = 0 kg-m/s

total momentum prior to collision = 10 000 + 0 = 10 000 kg-m/s

momentum after collision = 10 000 kg-m/s

mass now = 1 000 kg+2 000 kg = 3 000 kg

10 000 = 3 000 kg* velocity m/s

10 000/3 000 = velocity

3.33 m/s = velocity after collision

an impulse is a force applied over time , momentum is exclusive of external forces and a perfect collision is implied