Answer:
Explanation:
<u>1) Data:</u>
a) T = 25°C = 25 + 273.15K = 298.15 K
b) P = 1 atm
c) assumption: ideal gas
<u>2) Formulae and principles</u>
a) Ideal gas equation: p V = n R T, where:
- p = pressure
- V = volume
- n = number of moles
- R = universal constant of gases = 0.0821 atm-liter / K-mol
- T = absolute temperature (Kelvin)
b) Molar volume: ν = V / n, where:
- ν = molar volume
- V = volume
- n = number of moles
<u>3) Solution:</u>
- p V = n R T⇒ V/n = ν = RT / p =
= 0.0821 atm-liter / mol-K × 298.15 K / 1 atm
= 24.5 liter / mol
How many grams of glucose is dissolved in 2.88% glucose solution if 1944 grams of water is used???? The answer is C. 56 grams
<span>KCl<span>O3</span><span>(s)</span>+Δ→KCl<span>(s)</span>+<span>32</span><span>O2</span><span>(g)</span></span>
Approx. <span>3L</span> of dioxygen gas will be evolved.
Explanation:
We assume that the reaction as written proceeds quantitatively.
Moles of <span>KCl<span>O3</span><span>(s)</span></span> = <span><span>10.0⋅g</span><span>122.55⋅g⋅mo<span>l<span>−1</span></span></span></span> = <span>0.0816⋅mol</span>
And thus <span><span>32</span>×0.0816⋅mol</span> dioxygen are produced, i.e. <span>0.122⋅mol</span>.
At STP, an Ideal Gas occupies a volume of <span>22.4⋅L⋅mo<span>l<span>−1</span></span></span>.
And thus, volume of gas produced = <span>22.4⋅L⋅mo<span>l<span>−1</span></span>×0.0816⋅mol≅3L</span>
Note that this reaction would not work well without catalysis, typically <span>Mn<span>O2</span></span>.
The answer would be 425.599 because 1 ATM is 760 mmHg.
Answer: 100C of heat is needed.
Explanation: That is the heating point of water
