Answer:
The answer is 4
Explanation:
You divide the grams by the volume which will give you the density
so 19.2 divided by 4.8 equals 4
Answer:
According to <em>collision theory, to preventing a dangerous reaction from occurring</em>, <em>the best is to </em><em>keep reactants in separate containers</em> (last statement).
Justification:
<em>Collison theory</em> states that the the reactant substances (atoms, ions or molecules) must first collide to react and form the products.
Additionally, to form the products, the collisions must meet two requirements:
- the reactant substances must collide with the correct orientation, and
- the reactant substances must collide with energy enough to form the activated complex (transition state).
Hence, the <em>collision theory</em> permits you <em>preventing a dangerous reaction from occurring</em>, by using the elemental knowledge that the substances must first collide in order to they react, and so the most effective way is to keep the reactants in separate contaners, preventing the reactants from coming into direct contact.
Answer: a. 79.6 s
b. 44.3 s
c. 191 s
Explanation:
Expression for rate law for first order kinetics is given by:
where,
k = rate constant
t = age of sample
a = let initial amount of the reactant
a - x = amount left after decay process
a) for completion of half life:
Half life is the amount of time taken by a radioactive material to decay to half of its original value.
b) for completion of 32% of reaction
c) for completion of 81 % of reaction
Answer:
The final pressure of the gas mixture after the addition of the Ar gas is P₂= 2.25 atm
Explanation:
Using the ideal gas law
PV=nRT
if the Volume V = constant (rigid container) and assuming that the Ar added is at the same temperature as the gases that were in the container before the addition, the only way to increase P is by the number of moles n . Therefore
Inicial state ) P₁V=n₁RT
Final state ) P₂V=n₂RT
dividing both equations
P₂/P₁ = n₂/n₁ → P₂= P₁ * n₂/n₁
now we have to determine P₁ and n₂ /n₁.
For P₁ , we use the Dalton`s law , where p ar1 is the partial pressure of the argon initially and x ar1 is the initial molar fraction of argon (=0.5 since is equimolar mixture of 2 components)
p ar₁ = P₁ * x ar₁ → P₁ = p ar₁ / x ar₁ = 0.75 atm / 0.5 = 1.5 atm
n₁ = n ar₁ + n N₁ = n ar₁ + n ar₁ = 2 n ar₁
n₂ = n ar₂ + n N₂ = 2 n ar₁ + n ar₁ = 3 n ar₁
n₂ /n₁ = 3/2
therefore
P₂= P₁ * n₂/n₁ = 1.5 atm * 3/2 = 2.25 atm
P₂= 2.25 atm
