A 4.03 g sample of nitrogen gas has a volume of 921 milliliters at a pressure of 3.19 atm. The temperature of the N2 gas sample is:.

249 K

Explanation:

Step 1: Given data

Step 2: Calculate the moles corresponding to 4.03 g of nitrogen

The molar mass of N₂ is 28.01 g/mol.

4.03 g × 1 mol/28.01 g = 0.144 mol

Step 3: Calculate the temperature of the gas sample

We will use the ideal gas equation.

P × V = n × R × T

T = P × V / n × R

T = 3.19 atm × 0.921 L / 0.144 mol × 0.0821 atm.L/mol.K

T = 249 K

(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