Acquired because you don't inherit a "cut off" finger. You do it yourself.....if your clumsy enough
Answer:
64,433.6 Joules
Explanation:
<u>We are given</u>;
- Volume of water as 220 mL
- Initial temperature as 30°C
- Final temperature as 100°C
- Specific heat capacity of water as 4.184 J/g°C
We are required to calculate the amount of heat required to raise the temperature.
- We know that amount of heat is calculated by;
Q = mcΔT , where m is the mass, c is the specific heat, ΔT is the change in temperature.
Density of water is 1 g/mL
Thus, mass of water is 220 g
ΔT = 100°C - 30°C
= 70°C
Therefore;
Amount of heat, Q = 220g × 4.184 J/g°C × 70°C
= 64,433.6 Joules
Thus, the amount of heat required to raise the temperature of water is 64,433.6 Joules
Answer:
285g of fluorine
Explanation:
To solve this problem we need to find the mass of Freon in grams. Then, with its molar mass we can find moles of freon and, as 1 mole of Freon, CCl₂F₂, contains 2 moles of fluorine, we can find moles of fluorine and its mass:
<em>Mass Freon:</em>
<em>2.00lbs * (454g / 1lb) = </em>908g of Freon
<em>Moles freon -Molar mass: 120.91g/mol- and moles of fluorine:</em>
908g of Freon * (1mol / 120.91g) =
7.5 moles of freon * (2moles Fluorine / mole Freon): 15 moles of fluorine
<em>Mass fluorine -Atomic mass: 19g/mol-:</em>
15 moles F * (19g / mol) =
<h3>285g of fluorine</h3>
<span>Potassium and rubidium as they are in the same periodic table group as Na</span>
