look at the chemical tables. but i believe it is A
<h2>Hello!</h2>
The answer is: C2H6
<h2>Why?</h2>
First, we need to find the empirical formula of the compound:
Looking for the relative atomic mass for each element:
Finding the number of moles for each element:
Then, we need to determinate the mole ratio by dividing each result into the smallest number:
So, the empirical formula would be CH3
We are given the molar mass of the compound is equal to 30 g/mol
We need to compare the empirical formula molecular mass and the molecular formula molar mass in order to find the number of atoms of the compound:
Empirical formula molar mass:
Molecular formula molar mass = 30.0 g/mol
So, by dividing the molecular formula molar mass by the empirical formula molar mass we have the number of atoms of the compound:
Therefore,
The molecular formula will be: (CH3)2= C2H6
Have a nice day!
<u>Answer:</u>
<em>The substance is NaOH</em>
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<u>Explanation:</u>
To find the number of atoms of each element we multiply coefficient and the subscript
For example contains
5 × 1 = 5,Ca atoms and
5 × 2 = 10, Cl atoms
Sodium hydroxide is NaOH which contains
1, Na atom and
1, O atom and
1, H atom
Hence the ratio is 1 : 1 : 1
Answer:
For N₂F₂:
Molar fraction = 0.84
Partial pressure = 1.12 atm
For SF₄:
Molar fraction = 0.16
Partial pressure = 0.208 atm
Explanation:
It seems your question is missing the values required to solve the problem. However, an internet search showed me the following values for your question. If the values in your problem are different, your answer will be different as well, however the solving method will remain the same:
" A 5.00L tank at 0.7°C is filled with 16.5g of dinitrogen difluoride gas and 5.00g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. "
First we calculate the moles of each gas, using their molar mass:
- 16.5 g N₂F₂ ÷ 66 g/mol = 0.25 mol N₂F₂
- 5.00 g SF₄ ÷ 108 g/mol = 0.0463 mol SF₄
Total mol number = 0.25 + 0.0463 = 0.2963 mol
- Mole Fraction N₂F₂ = 0.25/0.2963 = 0.84
- Mole Fraction SF₄ = 0.0463/0.2963 = 0.16
Now we <u>use PV=nRT to calculate the partial pressure of each gas</u>:
P = ?
V = 5.00 L
T = 0.7 °C ⇒ 0.7 + 273.16 = 273.86 K
For N₂F₂:
- P * 5.00 L = 0.25 mol * 0.082 atm·L·mol⁻¹·K⁻¹ * 273.86 K
For SF₄:
- P * 5.00 L = 0.0463 mol * 0.082 atm·L·mol⁻¹·K⁻¹ * 273.86 K