I would say physical, because a physical change is affecting the form of a chemical substance, but not it's chemical makeup.
Answer:
pH = 6.8124
Explanation:
We know pH decreases with increase in temperature.
At room temperature i.e. 25⁰c pH of pure water is equal to 7
We know
Kw = [H⁺][OH⁻]...............(1)
where Kw = water dissociation constant
At equilibrium [H⁺] = [OH⁻]
So at 37⁰c i.e body temperature Kw = 2.4 × 10⁻¹⁴
From equation (1)
[H⁺]² = 2.4 × 10⁻¹⁴
[H⁺] = √2.4 × 10⁻¹⁴
[H⁺] = 1.54 × 10⁻⁷
pH = - log[H⁺]
= - log{1.54 × 10⁻⁷}
= 6.812
It would be C / Quantitative
The mass of carbon in 1 liter of mixture = 1.108 g
<h3>What is the mass of carbon in 1 liter of the mixture?</h3>
The mass of carbon in 1 liter of the mixture is determined as follows:
First the moles of gas is determined using the ideal gas formula:
n = (1 * 1)/(0.08205L * 298)
n = 0.0409 mole of total gas
mass of gas is then determined using the formula:
mass = 1 * 1.375
mass = 1.375 g
Let x = mass of CH₄ and y = mass of C₄H₁₀
x + y = 1.375 g
nCH₄ + nC₄H₁₀ = ntotat
moles = mass/molar mass
x + y = 1.695 => y = 1.695 - x
(x/molar mass of CH₄) + [(1.375 - x)/ molar mass C₄H₁₀ = 0.0409
x/16 + (1.375 - x)/58 = 0.0409
x = 0.380 g CH₄
y = 1.375 - 0.380
y = 0.995 g of C₄H₁₀
mass of C in CH₄ = 12/16 * 0.380 = 0.285
mass of C in C₄H₁₀ = 48/58 * 0.995 = 0.823
Mass of carbon in 1 liter of mixture = 0.285 + 0.823
Mass of carbon in 1 liter of mixture = 1.108 g
In conclusion, the carbon is the major component in the mixture.
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Answer:
0.214 L
Explanation:
Step 1: Write the balanced equation
This is a single displacement reaction.
Zn(s) + 2 HCl(aq) ⇒ ZnCl₂(aq) + H₂(g)
Step 2: Calculate the moles corresponding to 0.625 g of Zn
The molar mass of Zn is 65.38 g/mol.
0.625 g × 1 mol/65.38 g = 9.56 × 10⁻³ mol
Step 3: Calculate the moles of H₂ produced from 9.56 × 10⁻³ moles of Zn
The molar ratio of Zn to H₂ is 1:1. The moles of H₂ produced are 1/1 × 9.56 × 10⁻³ mol = 9.56 × 10⁻³ mol.
Step 4: Calculate the volume occupied by 9.56 × 10⁻³ moles of hydrogen
Assuming standard pressure and temperature, 1 mole of hydrogen occupies 22.4 L.
9.56 × 10⁻³ mol × 22.4 L/1 mol = 0.214 L
