True
True. In a collision, unbelted rear-seat occupants can be propelled forward at high speeds, becoming projectiles that can strike front-seat passengers. This increases the risk of severe injury or death for those in the front due to the additional force and impact. Seat belts are crucial for minimizing these risks for all occupants in a vehicle.
In a collision, unbelted rear seat occupants can be propelled forward at high speeds, acting as projectiles that may collide with front seat passengers. This phenomenon significantly increases the risk of severe injury or death for those in the front seats, as the force of the impact can be devastating. Proper seatbelt use is crucial to ensure the safety of all passengers in a vehicle, as it helps to secure occupants in place during a crash.
True. In a collision, unbelted rear seat occupants can be thrown forward at high speeds, potentially striking front seat passengers. This can lead to severe injuries or fatalities for those in the front, significantly increasing their risk during a crash. Proper seatbelt use for all passengers is crucial in minimizing these risks.
In a collision, unbelted rear-seat occupants can be propelled forward at high speeds, becoming dangerous projectiles that can strike front-seat passengers. This significantly increases the risk of injury or death for those in the front, as the force of the impact can cause severe trauma. Seat belts are crucial for all passengers, as they help to mitigate these risks by keeping occupants secured within their seats during a crash.
They move faster, number of collision increases,also the temperature increases.
increasing concentration increases rate of reaction as there are more particles so there is a larger chance of collision,it increases the probability of collision of the reactants.
increasing concentration increases rate of reaction as there are more particles so there is a larger chance of collision,it increases the probability of collision of the reactants.
Increases
rear-end
A Router
Increasing the concentration increases the molecules' collision frequency.
Decreasing particle size increases the surface area available for collision, leading to a higher collision frequency of reactants. Smaller particles move more freely and are more likely to collide with each other, increasing the chance of successful collisions and promoting faster reaction rates.