Convert the given density in mg/dL into a quantity with unit of g/L. This is shown below,
(200 mg / dL) x (10 dL / L) x (1 g / 1000 mg) = 2 g/L
Multiplying this quantity with the volume given, 5L, gives an answer of 10g.
Answer:
3 × 10⁴ kJ
Explanation:
Step 1: Write the balanced thermochemical equation
C₃H₈(g) + 5 O₂(g) ⟶ 3 CO₂(g) + 4 H₂O(g) ΔH = -2220 kJ
Step 2: Calculate the moles corresponding to 865.9 g of H₂O
The molar mass of H₂O is 18.02 g/mol.
865.9 g × 1 mol/18.02 g = 48.05 mol
Step 3: Calculate the heat produced when 48.05 moles of H₂O are produced
According to the thermochemical equation, 2220 kJ of heat are evolved when 4 moles of H₂O are produced.
48.05 mol × 2220 kJ/4 mol = 2.667 × 10⁴ kJ ≈ 3 × 10⁴ kJ
Answer:
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Explanation:
Answer:
The concentration of HCONH2 in equilibrium is 0.55M
Explanation:
Answer:
Ehthalpy change for the reaction is -323 kJ
Explanation:
Enthalpy change for a reaction, is given as:
Where and represents average bond energy in breaking "i" th bond and forming "j" th bond respectively. and are number of moles of bond break and form respectively.
Reaction:
Here, 2 moles of O-F bond and 2 moles of of O-H bond are broken
1 mol of O=O and 2 moles of H-F bonds are formed.
So,
So,