Answer:
3). 1.30 × 10^(24) molecules
Explanation:
From avogadro's law which state that equal volume of all gases at the same temperature and pressure contain the same number of molecules.
We can relate it to this question as;
V₁/n₁ = V₂/n₂
Where;
V₁ is initial volume
n₁ is initial number of molecules
V₂ is final volume
n₂ is final number of molecules
Thus at STP, we have V₁ = V₂ and as such Plugging in the relevant values gives;
5/(1.30 x 10^(24)) = 5/n₂
n₂ = 1.30 x 10^(24) molecules
Answer:
There are two types of mixtures: heterogeneous and homogeneous. Heterogeneous mixtures have visually distinguishable components, while homogeneous mixtures appear uniform throughout. The most common type of homogenous mixture is a solution, which can be a solid, liquid, or gas.
Hope this helped :)
D. a satellite orbiting Earth
Answer:
179 L of CO2
Explanation:
Given the equation of the reaction;
C2H6(g) + 7/2 O2(g) -------> 2CO2(g) + 3H2O(g)
Now 1 mole of ethane yields 2 moles of CO2 from the balanced reaction equation
1 mole of a gas occupies 22.4 L volume so,
22.4 L of ethane yields 44.8 L of CO2
89.5 L of ethane yields 89.5 * 44.8/22.4 = 179 L of CO2
In order to determine the increase in boiling point of a solvent due to the presence of a solute, we use the formula:
ΔT = Kb * m * i
Here, Kb is a property of the solvent, so remains constant regardless of the solute. Moreover, because the concentration m has been fixed, this will also not be considered. In order to determine which solute will have the greatest effect, we must check i, the van't Hoff factor.
Simply stated, i is the number of ions that a substance produces when dissolved. Therefore, the solute producing the most ions will be the one causing the greatest change in boiling point temperature.