Answer:
C₄F₈
Explanation:
Using their mole ratio to compute their mass
molar mass of carbon = 12.0107 g/mol
molar mass of fluorine gas = 37.99681
let x = mass of carbon
given mass of fluorine = 1.70 g
x / 12.01067 = 1.70 / 37.99687
cross multiply
x = ( 1.70 × 12) / 37.99687 = 20.4 / 37.99687 = 0.53688 g
mass of one mole of CF₂ = 0.53688 + 1.70 = 2.23688 g
number of mole of CF₂ = 8.93 g / 2.23688 = 3.992 approx 4
molecular formula of CF₂ = 4 (CF₂) = C₄F₈
Hello. You have not presented the image that presents the two elements mentioned in the question. This makes it impossible for your question to be answered. However, I will try to help you as best I can.
To say whether the compounds obey the law of multiple proportions, you should observe whether one of the elements, formed from the compounds, maintains a fixed mass, while the other element presents the mass in a varied amount of small, whole numbers, spread across the formed compounds .
This is because the law of multiple proportions states that an element must have a fixed mass when reacting with another element to create compounds. This reaction will allow this element to keep the mass fixed, while the other element will generate different compounds, where each one presents a part of the mass of the forming element, in small and whole numbers.
Explanation:
Chromosomal DNA is packaged inside microscopic nuclei with the help of histones. These are positively-charged proteins that strongly adhere to negatively-charged DNA and form complexes called nucleosomes. Each nuclesome is composed of DNA wound 1.65 times around eight histone proteins.
The number of proton in the nucleus of an atom is its Atomic Number.
Answer:
CO(g) + H₂O(g) <=> CO₂(g) + H₂(g), (volume is decreased) .. No effect.
PCl₃(g) + Cl₂(g) <=> PCl₅(g)
, (volume is increased) .. Shift left.
CaCO₃(s) <=> CaO(s) + CO₂(g)
, (volume is increased) .. Shift right.
Explanation:
<em>Le Châtelier's principle</em><em> states that when there is an dynamic equilibrium, and this equilibrium is disturbed by an external factor, the equilibrium will be shifted in the direction that can cancel the effect of the external factor to reattain the equilibrium.</em>
<em />
<em>CO(g) + H₂O(g) <=> CO₂(g) + H₂(g) (volume is decreased)</em>
- When volume is decreased, the pressure will increase:
- When there is an increase in pressure, the equilibrium will shift towards the side with fewer moles of gas of the reaction. And when there is a decrease in pressure, the equilibrium will shift towards the side with more moles of gas of the reaction.
- The reactants side (left) has 2.0 moles of gases and the products side (right) has 2.0 moles of gases.
So, decreasing the volume will have no effect on the reaction.
<em>PCl₃(g) + Cl₂(g) <=> PCl₅(g)
, (volume is increased)</em>
- When volume is increased, the pressure will decrease:
- When there is an decrease in pressure, the equilibrium will shift towards the side with more moles of gas of the reaction.
- The reactants side (left) has 2.0 moles of gases and the products side (right) has 1.0 mole of gases.
- So, decreasing the pressure will shift the reaction to the side with more moles of gas (left side).
so, increasing the volume will shift the reaction left.
<em>CaCO₃(s) <=> CaO(s) + CO₂(g)
, (volume is increased)</em>
- When volume is increased, the pressure will decrease:
- When there is an decrease in pressure, the equilibrium will shift towards the side with more moles of gas of the reaction.
- The reactants side (left) has 0 moles of gases and the products side (right) has 1.0 mole of gases.
- So, decreasing the pressure will shift the reaction to the side with more moles of gas (right side).
so, increasing the volume will shift the reaction right.