Answer:
So the empirical formula is C14H18N2O5
Explanation:
C = 57.2% = 12g/mol
H = 6.1% = 1g/mol
N = 9.5% = 14g/mol
O = 27.2% = 16g/mol
Empirical Formula for compound hmm
Assume
C = 57.2g
H = 6.1g
N = 9.5g
O = 27.2g
So we have
C = 57.2g/12g = 4.76 moles
H = 6.1g/1g = 6.10 moles
N = 9.5g/14g = 0.68 moles
O = 27.2g/16g = 1.70 moles
Divide each mole value by the smallest number of moles calculated. Round to the nearest whole number.
C = 4.76 moles / 0.68 moles = 7
H = 6.10 moles / 0.68 moles = 9
N = 0.68 moles / 0.68 moles = 1
O = 1.70 moles / 0.68 moles = 2.5
Ok so we now have the ratios but for O it's 2.5, have to be whole numbers so we will need to double all the numbers.
C = 14
H = 18
N = 2
O = 5
So the empirical formula is C14H18N2O5
Answer:
3NH₄OH + H₃PO₄ → (NH₄)₃PO₄ + 3H₂O
Products are water and ammonium phosphate
Explanation:
This is a neutralization between a weak base and a weak acid where the products are water and the correspondent salt.
Base: NH₄OH → NH₄⁺ + OH⁻
Acid : H₃PO₄ → 3H⁺ + PO₄⁻³
H⁺ bonds to OH⁻ to make H₂O → As we have 3 protons, we can make 3 moles of water, so there are needed 3 OH⁻.
Phosphate has -3 as oxidation state, then it needs 3 ammonium to form the salt.
The balanced equation is:
3NH₄OH + H₃PO₄ → (NH₄)₃PO₄ + 3H₂O
Q= m*c*ΔT
⇒ 209 J= 10.0 g* 4.18 J/(g*C)* (x- 23.0 C)
⇒ ...
⇒ x= 28.0 C
(3) 28.0<span>°C is the correct answer.
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Hope this helps~
Answer:
C!
Explanation:
only C
A: solid B: liquid : C: GAS
