Answer:
oxygen and silicon, both are common
Answer:
i odnt knwonwta whyour sayong
Explanation:
Answer : The correct option is (A).
Explanation :
- Endothermic reaction : When two liquids are combine into a flask, then the flask feels cold when we touch it because the system absorbed heat from the surrounding.
In general, endothermic process absorbs heat and cool the surrounding.
- Exothermic reaction : When two liquids are combine into a flask, then the flask feels hot when we touch it because the system released heat into the surrounding.
In general, exothermic process releases heat and rise the temperature of surrounding.
Answer is: 588.15 <span>grams of ethanol.
</span>Chemical reaction: C₆H₁₂O₆ → 2C₂H₅OH + 2CO₂.
m(C₆H₁₂O₆) = 1150 g.
n(C₆H₁₂O₆) = m(C₆H₁₂O₆) ÷ M(C₆H₁₂O₆).
n(C₆H₁₂O₆) = 1150 g ÷ 180.16 g/mol.
n(C₆H₁₂O₆) = 6.38 mol.
From chemical reaction: n(C₆H₁₂O₆) : n(C₂H₅OH) = 1 : 2.
n(C₂H₅OH) = 12.76 mol.
m(C₂H₅OH) = 12.76 mol · 46.07 g/mol.
m(C₂H₅OH) = 588.15 g.
Answer:
Moles of boron trifluoride gas that were collected = 11.6 mol
Mass of boron trifluoride gas that were collected = 787 g
Explanation:
Given that:
Temperature = 2.0 °C
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T = (2.0 + 273.15) K = 275.15 K
V = 15.0 L
Pressure = 0.130 atm
Using ideal gas equation as:
where,
P is the pressure
V is the volume
n is the number of moles
T is the temperature
R is Gas constant having value = 0.0821 L atm/ K mol
Applying the equation as:
0.130 atm × 15.0 L = n ×0.0821 L atm/ K mol × 275.15 K
⇒n = 11.6 mol
<u>Thus, Moles of boron trifluoride gas that were collected = 11.6 mol
</u>
Molar mass of boron trifluoride gas = 67.82 g/mol
The formula for the calculation of moles is shown below:
Thus,
<u>Mass of boron trifluoride gas that were collected = 787 g</u>