Answer:
11.45kcal/g
2.612 × 10³ kcal
Explanation:
When a compound burns (combustion) it produces carbon dioxide and water. The combustion of 2-methylheptane can be represented by the following balanced equation:
2 C₈H₁₈ + 25 O₂ ⇄ 16 CO₂ + 18 H₂O
It releases 1.306 × 10³ kcal every 1 mol of C₈H₁₈ that is burned.
<em>What is the heat of combustion for 2-methylheptane in kcal/gram?</em>
We know that the molar mass of C₈H₁₈ is 114.0g/mol. Then, using proportions:
<em>How much heat will be given off if molar quantities of 2-methylheptane react according to the following equation? 2 C₈H₁₈ + 25 O₂ ⇄ 16 CO₂ + 18 H₂O</em>
In this equation we have 2 moles of C₈H₁₈. So,
Answer:
a) <u>Balanced Equation</u>
2NaCl (aq) + (NH₄)₂CO₃ (aq) → Na₂CO₃ (aq) + 2NH₄Cl (aq)
b) <u>Total Ionic Equation</u>
2Na⁺ (aq) + 2Cl⁻ (aq) + 2NH₄⁺ (aq) + CO₃ ²⁻ (aq) → 2Na⁺ (aq) + CO₃²⁻ (aq) + 2NH₄⁺ (aq) + 2Cl⁻ (aq)
c) <u>Net Ionic Equation</u>
All are spectator ions, so no net ionic equation.
D. ( Neither ultrasonic nor infrasonic vibrations can be heard by humans. )
Im guessing it would be 3.53 × 1023 atoms
Answer:
346.g of solution
Explanation:
In this case, if we have 5.2 % by mass it means that in <u>100 g of the solution we will have 5.2 g of glucose</u>. Therefore we can do the calculation:
<u>5.2 g of glucose = 100 g of solution</u>
So, if we need 8 g of glucose we had to have 346.15 g of solution
This logic can work for all types of solutions. By mass (as in this case), by volume or mass/volume.
I hope it helps!
