Answer:
Option A. 107 mL
Explanation:
From the question given above, the following data were obtained:
Initial volume (V₁) = 150 mL
Initial pressure (P₁) = 500 mmHg
Final pressure (P₂) = 700 mmHg
Temperature = constant
Final volume (V₂) =?
The final volume of the gas can be obtained by using the Boyle's law equation as shown below:
P₁V₁ = P₂V₂
500 × 150 = 700 × V₂
75000 = 700 × V₂
Divide both side by 700
V₂ = 75000 / 700
V₂ = 107 mL
Therefore, the final volume of the gas is 107 mL.
Answer:
40 moles of O₂
30 moles of CO₂
Explanation:
Given parameters:
Number of moles of C₃H₄ = 10moles
Unknown:
Number of moles of CO₂ = ?
Solution:
The number of moles helps to understand and make quantitative measurements involving chemical reactions.
We start by solving this sort of problem by ensuring that the given equation is properly balanced;
C₃H₄ + 4O₂ → 3CO₂ + 2H₂O
We can clearly see that all the atoms are conserved.
Now, we work from the known to unknown. We know the number of moles of C₃H₄ to be 10moles;
1 mole of C₃H₄ reacted with 4 moles of O₂
10 moles of C₃H₄ will react with 10 x 4 = 40moles of O₂
1 mole of C₃H₄ will produce 3 moles of CO₂
10 moles of C₃H₄ will produce 10 x 3 = 30moles of CO₂
The answer is Strontium(Sr). The reactive increase from right to left. And this element has two valence electrons. So Rb is not correct. Then the very reactive metal is Sr.
Answer: 2HCO + 4O → H2 + 2CO3
Explanation: Oxomethyl + Oxygen = Dihydrogen + Carbon Trioxide
Reaction Type: SINGLE REPLACEMENT
***If you found my answer helpful, please give me the brainliest, please give a nice rating, and the thanks ( heart icon :) ***
