Answer:
1) 0.009 61 g C; 2) 0.008 00 mol C
Step-by-step explanation:
You know that you will need a balanced equation with masses, moles, and molar masses, so gather all the information in one place.
M_r: 12.01 44.01
C + ½O₂ ⟶ CO₂
m/g: 0.352
1) <em>Mass of C
</em>
Convert grams of CO₂ to grams of C
44.01 g CO₂ = 12.01 g C
Mass of C = 0.352 g CO₂ × 12.01 g C/44.01 g CO₂
Mass of C = 0.009 61 g C
2) <em>Moles of C
</em>
Convert mass of C to moles of C.
1 mol C = 12.01 g C
Moles of C = 0.00961 g C × (1 mol C/12.01 g C)
Moles of C = 0.008 00 mol C
All the carbon comes from Compound A, so there are 0.008 00 mol C in Compound A.
Answer:
The mass of heavier isotope is 345.6 amu.
Explanation:
Given data:
atomic wight of compound = 342.38 amu
lighter isotope mass = 340.91 amu
abundance of lighter isotope = 68.322%
mass of heavier isotope = ?
Solution:
average atomic mass = ( % age abundance of lighter isotope × its atomic mass) + (% age abundance of heavier isotope × its atomic mass) / 100
percentage of heavier isotope = 100- 68.322 = 31.678
Now we will put the values in formula.
342.38 = (68.322× 340.91) + (31.678 × X) / 100
342.38 = 23291.65302 + (31.678 × X) / 100
342.38 × 100 = 23291.65302 + (31.678 × X)
34238 -23291.65302 = (31.678 × X)
10946.35 / 31.678 = X
345.6 = X
The mass of heavier isotope is 345.6 amu.
Hydrogen is actually a combustible gas. But when you try to burn it, it explodes. However when you produce hydrogen in a laboratory, which is relatively less, and put a burning splint, it also explodes, but in a reduced form - a <span>POP </span><span>sound. The very small explosion (doesn't feel like one, does it?) extinguishes the flame.</span>
Answer:
Hi! Think of it like this:
You and your family are going to go on a vaction for the holidays, to south america or somewhere else. You´re near the equator so it will be warm. If you were to move there, you might pull out the swimsiutes because most of the time, its useally warm and sunny. They dont really get cold weather. They will have a nice and warm christmas.
The fuel released 90 calories of heat.
Let suppose that water experiments an entirely <em>sensible</em> heating. Hence, the heat released by the fuel is equal to the heat <em>absorbed</em> by the water because of principle of energy conservation. The heat <em>released</em> by the fuel is expressed by the following formula:
(1)
Where:
- Mass of the sample, in grams.
- Specific heat of water, in calories per gram-degree Celsius.
- Temperature change, in degrees Celsius.
If we know that 
, 
and 
, then the heat released by the fuel is:
The fuel released 90 calories of heat.
We kindly invite to check this question on sensible heat: brainly.com/question/11325154
