Answer is: 0,250 atm.
T₁(chlorine) = 27°C = 300K.
T₂(chlorine) = 227°C = 500K.
T₂/T₁ = 1,66.
p1(chlorine) = 0,150 atm.
p2(chlorine) = ?
V(chlorine) = constant.
n(chlorine) = 0,0200 mol.
R - gas constant, R = 0.0821 atm·l/mol·K.
Ideal gas law: p·V = n·R·T.
p = n·R·T÷V.
If temperature was increased 1,66 times, pressure also increase 1,66 times: 1,66·0,150 atm = 0,250 atm.
Answer:
1.50 × 10²⁴ atoms C
Explanation:
Step 1: Define
Molar mass of C - 12.01 g/mol
Avagadro's Number: 6.02 × 10²³ atoms, molecules, formula units, etc.
Step 2: Use Dimensional Analysis
= 1.50375 × 10²⁴ atoms C
Step 3: Simplify
We are given 3 sig figs.
1.50375 × 10²⁴ atoms C ≈ 1.50 × 10²⁴ atoms C
Answer:
pH of 7.86, then the [OH-] is equal to 10^(14-7.86) = 10^6.14 M
Explanation:
