We have:
V = 55.0 gallons x 3.78541 = 208 L
P = 16500 kPa
T = 23 + 273.15 = 296.15 K
Part A) From the equation PV =
![\frac{mRT}{M}](https://tex.z-dn.net/?f=%20%5Cfrac%7BmRT%7D%7BM%7D%20)
we get:
mass of O₂ = (16500 kPa x 208 L x 32 g/mol) / (8.314 x 296.15 K)
= 44.6 Kg
Part B) at STP we have:
T = 273.15 K and P = 101.3 kPa
so from PV = mRT / M
V = (44600 x 8.314 x 273.15) / (32 x 101.3)
= 31248 L
Part C) From the equation PV = mRT / M
we get
T = (150 atm x 101.3 kPa / atm x 208L x 32g/mol) / (8.314 x 44600)
= 272.8 K
Part D) we have:
T = 24 + 273.15 K = 297.15 K
so from PV = mRT / M, we get
P = (44600 x 8.314 x 297.15) / (32 x 55)
= 62464 kPa
Answer:
7 moles of water will produced from 3.5 moles of ammonium nitrate.
Explanation:
Given data:
Moles of ammonium nitrate = 3.5 mol
Moles of water produced = ?
Solution:
Chemical equation:
2NH₄NO₃ → 2N₂ + 4H₂O + O₂
Now we will compare the moles of ammonium nitrate with water.
NH₄NO₃ : H₂O
2 : 4
3.5 : 4/2×3.5 = 7 moles
Thus 7 moles of water will produced from 3.5 moles of ammonium nitrate.
Phenolphthalein turns pink when mixed with bases; since Mg(OH)2 is the only base, it is the answer.
Answer:
The specific heat of the mineral is 0.1272J/g°C
Explanation:
The sample is given energy to the calorimeter and the sample of water.
The energy released for the sample is equal to the energy absorbed for both the calorimeter and the water:
C(Sample)*m*ΔT = C(Calorimeter)*ΔT + C(water)*m*ΔT
<em>Where C is specific heat</em>
<em>m is mass of the sample and water</em>
<em>And ΔT is change in temperature</em>
<em />
C(Sample)*149g*(92.7°C-23.7°C) = 12.8J/K*(23.7°C-20.0°C) + 4.184J/g°C*81.4g*(23.7°C-20.0°C)
C(Sample)*10281g°C = 47.36J + 1260.1J
C(Sample) = 0.1272J/g°C
<h3>The specific heat of the mineral is 0.1272J/g°C</h3>
<em />
Answer:
The mass of NaHCO3 required is 235.22 g
Explanation:
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Continuation of Question:
2NaHCO3(s) + H2SO4(aq) → Na2SO4(aq) + 2CO2(g) + 2H2O(l)
You estimate that your acid spill contains about 1.4 mol H2SO4. What mass of NaHCO3 do you need to neutralize the acid?
********\
The question requires us to calculate the mass of NaHCO3 to neutralize the acid.
From the balanced chemical equation;
1 mol of H2SO4 requires 2 mol of NaHCO3
1.4 would require x?
Upon solving for x we have;
x = 1.4 * 2 = 2.8 mol of NaHCO3
The relationship between mass and number of moles is given as;
Mass = Number of moles * Molar mass
Mass = 2.8 mol * 84.007 g/mol
Mass = 235.22 g