According to my calculations the correct Answer is C. +694. The answers A B and D Are incorrect. It cannot be A because I said it also cannot be B because C=H. The answer would not be D because balls in your jaws = +1192 And the answer will be CORRECT ANSWER C=+694
Answer:
The answer to your question is below
Explanation:
There are 4 types of chemical reactions:
- Synthesis is when two elements or compounds form only one compound.
- Decomposition is when 1 compound is broken into 2 or more products.
- Single replacement is when one element is replaced by another element.
- Double replacement is when the cations of two compounds are interchanged.
1.- Decomposition 2 Al₂O₃ ⇒ 4 Al + 3O₂
2.- Single replacement Mg + 2HNO₃ ⇒ Mg(NO₃)₂ + H₂
3.- Combustion 2C₆H₆ + 15O₂ ⇒ 12CO₂ + 6H₂O
4.- Synthesis 2Ag + S ⇒ Ag₂S
5.- Double replacement 3Ca(OH)₂ + 2H₃PO₄ ⇒ Ca₃(PO₄)₂ + 6 H₂O
Answer:
1. The empirical formula => C₆H₁₀OS₂
2. Molecular formula => C₃₆H₆₀O₆S₁₂
Explanation:
1. Determination of the empirical formula.
Carbon (C) = 2.96 g
Hydrogen (H) = 0.414 g
Oxygen (O) = 0.675 g
Sulphur (S) = 2.96 g
Divide by their molar mass
C = 2.96 / 12 = 0.247
H = 0.414 / 1 = 0.414
O = 0.675 / 16 = 0.042
S = 2.96 / 32 = 0.0925
Divide by the smallest
C = 0.247 / 0.042 = 6
H = 0.414 / 0.042 = 10
O = 0.042 / 0.042 = 1
S = 0.0925 /0.042 = 2
Therefore, the empirical formula is
C₆H₁₀OS₂
2. Determination of the molecular formula.
Molar mass of compound = 972 g/mol
Empirical formula => C₆H₁₀OS₂
Molecular formula =>?
Molecular formula = [C₆H₁₀OS₂]ₙ
Molecular formula = molar mass of compound
Thus,
[C₆H₁₀OS₂]ₙ = 972
[(12×6) + (10×1) + 16 + (32×2)]n = 972
[72 + 10 + 16 + 64]n = 32
162n = 972
Divide both side by 162
n = 972 / 162
n = 6
Molecular formula = [C₆H₁₀OS₂]ₙ
Molecular formula = [C₆H₁₀OS₂]₆
Molecular formula = C₃₆H₆₀O₆S₁₂
Answer:
1550.8
Explanation:
This is the ideal gas equation:
PV=nRT
We can rearrange the ideal gas equation to solve for the pressure of the nitrogen gas.
P=nRT/ V
We can find the pressure of the nitrogen gas by plugging in the values for the moles of gas, temperature, and volume. Since we want the pressure in units of Torr we use the R value62.36358L Torr K−1 mol-1
P=nRT/ V
(0.316 mol )(62.36358 L*Torr/K*mol)(315 K) / 4.00 L =1550 Torr
The correct answer is 1550
