Describes how Anders Celsius devised the temperature scale that bears his name
1 answer:
You might be interested in
Answer:
E.F= OH
M.F=
Explanation:
Empirical Formula
Step 1: Calculate mols of each element
0.44gH(1 mol H/ 1.008g H)= 0.4365 mol H
*note leave extra sig figs for calculations
6.92gO(1 mol O/ 16 g O)=0.4325 mol O
Step 2: Identify which is the smallest mol
*in this case 0.4365 mol H> 0.4325 mol O so we will use 0.4325 mol O
Step 3: Divide above calculations by the smallest mol
0.4325 mol O/0.4325= 1
0.4365 mol H/0.4325= 1.009 *rounds to 1
Step 4: use calculations as subscripts
Oxygen = 1 so the subscript will 1 (O)
Hydrogen = 1 so the subscript will 1 (H)
making E.F= OH
Molecular Formula:
Step 1: identify molecular mass and mass from the E.F
the molecular mass is given 34.00g/mol
the mass of the E.F is
(oxygen mass from periodic table)+(hydrogen mass from periodic table)
16+1.008= 17.008
Step 2:Divide the molecular mass by the mass given by the emipirical formula.
round to 2
Step 3:Multiply the empirical formula (the subscripts) by this number to get the molecular formula. ANSWER: M.F=2(OH)-
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,