Answer:
Mass of water produced= 1.8 g
Explanation:
Given data:
Mass of water produced = ?
Mass of butane = 1.36 g
Mass of oxygen = excess
Solution:
Chemical equation:
2C₄H₁₀ +13 O₂ → 8CO₂ + 10H₂O
Number of moles of butane:
Number of moles = mass/molar mass
Number of moles = 1.36 g/ 58.12 g/mol
Number of moles = 0.02 mol
Now we will compare the moles of butane with water.
C₄H₁₀ : H₂O
2 : 10
0.02 : 10/2×0.02 = 0.1 mol
Mass of water produced:
Mass = molar mass × molar mass
Mass = 0.1 mol × 18 g/mol
Mass = 1.8 g
Answer:
161 mL
Explanation:
- Pb(NO₃)₂(aq) + Ba(OH)₂(aq) → Pb(OH)₂(s) + Ba(NO₃)₂(aq)
First we <u>calculate how many Pb⁺² moles reacted</u>, using the<em> given concentration and volume of the Pb(NO₃)₂ solution</em>:
- 163 mL * 0.656 M = 107 mmol Pb(NO₃)₂
As<em> 1 millimol of Pb(NO₃)₂ would react with 1 millimol of Ba(OH)₂,</em> to precipitate 107 mmoles of Pb(NO₃)₂ we would require 107 mmoles of Ba(OH)₂.
Using the number of moles and the concentration we can <u>calculate the required number of milliliters</u>:
- 0.666 M = 107 mmol / x mL
C + O2 ——> CO2
Carbon plus oxygen forms carbon dioxide
Answer:
second option and last option
Explanation:
Know how to do an electron configuration. This is correct because it adds up to 8 and is in the correct order.
All valence electrons are in the last shell. In this case, 2p is the last shell.
Answer: Option (e) is the correct answer.
Explanation:
According to Henry's Law, mass of a gas which will dissolve into a solution is directly proportional to the partial pressure of that gas above the solution.
Mathematically, C = 
where, 
= Henry's constant
P = partial pressure
Since, concentration is directly proportional to partial pressure of a gas. Hence, more is the partial pressure more will be the number of molecules present in the liquid.
Thus, we can conclude that the statement there are twice as many gas molecules in the liquid, is true.
