Answer:
We need 12.26 grams H2SO4
Explanation:
Step 1: Data given
Volume of a H2SO4 solution = 500 mL = 0.500 L
Concentration of the H2SO4 solution = 0.250 M
Molar mass of H2SO4 = 98.08 g/mol
Step 2: Calculate moles H2SO4
Moles H2SO4 = concentration * volume
Moles H2SO4 = 0.250 M * 0.500 L
Moles H2SO4 = 0.125 moles
Step 3: Calculate mass of H2SO4
Mass of H2SO4 = moles * molar mass
Mass of H2SO4 = 0.125 moles * 98.08 g/mol
Mass of H2SO4 = 12.26 grams
We need 12.26 grams H2SO4
Answer:flashover
Explanation: flashover are event that occurs when all of the combustible materials in a room reach their ignition temperatures at the same time
<em>It is beneficial because it provides stronger support for the evidence related to the discovery</em>
<u>Answer:</u> <em>The correct answer is the second option that is given with shows it is beneficial.</em>
<u>Explanation:</u>
The discovery of an element whose properties are known from before would make it easier for the scientists to know the properties of elements and its uses after the discovery of element.
Since the elements’ properties are already known as element that possesses these properties and will look forward to find that and once the element is found the element can be named and can be used directly, since its uses are already known.
Answer:
Molar concentration of S₂ is 1.77×10⁻⁶M
Explanation:
For the reaction:
2H₂S(g) ⇄ 2H₂(g) + S₂(g)
The equilibirum constant, K, is defined as:
<em>(1)</em>
Concentrations in equilibirum are:
[H₂S] : 0,163/0.500L - X
[H₂] : 0,0500/0.500L + X
[S₂] : X
Replacing the concentrations and the equilibrium value in (1):
![K = \frac{[X][0.1+X]^2}{[0326-X]^2}](https://tex.z-dn.net/?f=K%20%3D%20%5Cfrac%7B%5BX%5D%5B0.1%2BX%5D%5E2%7D%7B%5B0326-X%5D%5E2%7D)
1.67x10⁻⁷ = X (X² + 0.2X + 0.01) / (X² -0.652X + 0.106)
1.67x10⁻⁷X² - 1.09x10⁻⁷X + 1.77x10⁻⁸ = X³ + 0.2X² + 0.01X
0 = X³ + 0.2X² + 0.01X - 1.77x10⁻⁸
Solving for X:
X = 1.77×10⁻⁶
As [S₂] = X, <em>molar concentration of S₂ is 1.77×10⁻⁶M</em>
I hope it helps!