The answer is C. Aluminium since it is highly reactive
Answer:
1.429 g of N₂
Explanation:
The Haber process is a reaction that combines nitrogen with hydrogen to form ammonia according to the following balanced equation:
- N₂ ₍g₎ + 3 H₂ ₍g₎ ⇆ 2NH₃ ₍g₎
One can note that 1 mol of N₂ react with H₂ to produce 2 mol of NH₃.
We cannot compare weight of a substance (in grams) to another in chemical reactions, but we can use moles, then we have to convert the weight of NH3 to moles.
no. of moles of NH₃ = (mass / molar mass) = (1.7 g / 17 g/mol) = 0.1 mol
and the actual yield is 98% , then the theoretical number of moles that would be produced are:
- percent yield = (actual yield / theoretical yield) × 100
98 = (0.1 mol / theoretical yield) × 100
theoretical no. of moles of NH₃ = (0.1 * 100) /98 = 0.102 mol
using cross multiplication
1 mol of N₂ → 2 mol of NH₃.
?? mol of N₂ → 0.102 mol of NH₃.
no of moles of N₂ = [(1 mol * 0.102 mol) / 2 mol] = 0.051 mol
Last step is to convert the moles back to grams using:
mass = (no of moles of N₂ * molar mass of N₂)
= (0.051 mol * 28 g/mol) = 1.429 g
Answer:
The mass % of HNO3 in the solution is 71.0 %
Explanation:
Step 1: Data given
Density of HNO3 = 1.42 g/mL
Concentration = 16 M = 16 mol /L
Molar mass HNO3 = 63.01 g/mol
Assume the volume = 1L or 1000 mL
Step 2: Calculate mass of the solution
Mass = density * volume
Mass = 1.42 g/mL * 1000 mL
Mass = 1420 grams
Step 3: Calculate moles HNO3
Moles = molarity * volume
Moles = 16 M * 1L
Moles = 16 moles
Step 4: Calculate mass HNO3
Mass HNO3 = moles * molar mass
Mass HNO3 = 16.0 moles * 63.01 g/mol
Mass HNO3 = 1008.16 grams
Step 5: Calculate the mass percent
mass % = (1008.16 grams / 1420 grams) *100%
mass % = 71.0 %
The mass % of HNO3 in the solution is 71.0 %
i. The dissolution of PbSO₄ in water entails its ionizing into its constituent ions:
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ii. Given the dissolution of some substance
,
the Ksp, or the solubility product constant, of the preceding equation takes the general form
![K_{sp} = [B]^y [C]^z](https://tex.z-dn.net/?f=K_%7Bsp%7D%20%3D%20%5BB%5D%5Ey%20%5BC%5D%5Ez)
.
The concentrations of pure solids (like substance A) and liquids are excluded from the equilibrium expression.
So, given our dissociation equation in question i., our Ksp expression would be written as:
![K_{sp} = \mathrm{[Pb^{2+}] [SO_4^{2-}]}](https://tex.z-dn.net/?f=K_%7Bsp%7D%20%3D%20%5Cmathrm%7B%5BPb%5E%7B2%2B%7D%5D%20%5BSO_4%5E%7B2-%7D%5D%7D)
.
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iii. Presumably, what we're being asked for here is the <em>molar </em>solubility of PbSO4 (at the standard 25 °C, as Ksp is temperature dependent). We have all the information needed to calculate the molar solubility. Since the Ksp tells us the ratio of equilibrium concentrations of PbSO4 in solution, we can consider either [Pb2+] or [SO4^2-] as equivalent to our molar solubility (since the concentration of either ion is the extent to which solid PbSO4 will dissociate or dissolve in water).
We know that Ksp = [Pb2+][SO4^2-], and we are given the value of the Ksp of for PbSO4 as 1.3 × 10⁻⁸. Since the molar ratio between the two ions are the same, we can use an equivalent variable to represent both:
So, the molar solubility of PbSO4 is 1.1 × 10⁻⁴ mol/L. The answer is given to two significant figures since the Ksp is given to two significant figures.
Because the heat of the ocean mixed with the cold air above the ocean causes a hurricane
