Answer:
Explanation:
We are given the masses of two reactants and asked to determine the mass of the product.
This looks like a limiting reactant problem.
1. Assemble the information
We will need a balanced equation with masses and molar masses, so let’s gather all the information in one place.
MM: 114.23 32.00 44.01
2C₈H₁₈ + 25O₂ ⟶ 16CO₂ + 18H₂O
Mass/g: 10.3 69.
2. Calculate the moles of each reactant
3. Calculate the moles of CO₂ from each reactant
4. Calculate the mass of CO₂
The question mentions a change in temperature from 25 to 50 °C. With that, the aim of the question is to determine the change in volume based on that change in temperature. Therefore this question is based on Gay- Lussac's Gas Law which notes that an increase in temperature, causes an increase in pressure since the two are directly proportional (once volume remains constant). Thus Gay-Lussac's Equation can be used to solve for the answer.
Boyle's Equation:
=
Since the initial temperature (T₁) is 25 C, the final temperature is 50 C (T₂) and the initial pressure (P₁) is 103 kPa, then we can substitute these into the equation to find the final pressure (P₂).
=
∴ by substituting the known values, ⇒ (103 kPa) ÷ (25 °C) = (P₂) ÷ (50 °C)
⇒ P₂ = (4.12 kPa · °C) (50 °C)
=
206 kPa
Thus the pressure of the gas since the temperature was raised from 25 °C to 50 °C is
206 kPa
When one mole of Na3PO4.3H2O is heated extensively, three moles of water are released.
The water molecules in Na3PO4.3H2O are called molecules of water of crystallization. These molecules are not covalently bonded to the Na3PO4 molecule. They are only loosely attached to the substance.
Strong heating will drive away these molecules of water of crystallization to give three moles of water in the product.
Hence, when one mole of Na3PO4.3H2O is heated extensively, three moles of water are released.
Learn more: brainly.com/question/14252791
