Answer:
Explanation:
There are two heat flows in this process and, since energy (heat) can neither be destroyed nor created, the energy change for the system must equal zero.
Data:
For Fe, m₁ = ?; C₁ = 0.452 J°C⁻¹g⁻¹; Ti = 2.00 °C; T_f = 21.50 °C
For H₂O, m₂ = 120 g; C₂ = 4.18 J°C⁻¹g⁻¹; Ti = 22.00 °C; T_f = 21.50 °C
Calculations:
1. Temperature changes
ΔT₁ = T_f - Ti = 21.50 °C - 2.00 °C = 19.50 °C
ΔT₂ = T_f - Ti = 21.50 °C - 22.00 °C = -0.50 °C
2. Mass of steel rod
Answer:
Potential energy.
Explanation:
Potential energy is the energy in a body due to its position.
Answer:
No percent yield is actual yields/ theoretical yields .x 100%.
Explanation:
The theoretical yield is the maximum amount of product that could be formed from given amounts of products. The actual yield must be less than or equal to the theoretical theory.
Answer:
162g
Explanation:
We'll begin by writing the balanced equation for the reaction. This is given below:
2C2H6 + 7O2 —> 4CO2 + 6H2O
Next, we shall determine the number of mole of water, H2O produced by the reaction of 3 moles of C2H6.
This can be obtained as follow:
From the balanced equation above,
2 moles of C2H6 reacted to produce 6 moles of H2O.
Therefore, 3 moles of C2H6 will react to produce = (3 x 6)/2 = 9 moles of H2O.
Therefore, 9 moles of H2O is produced from the reaction.
Finally, we shall convert 9 moles of H2O to grams.
This can be done as shown below:
Molar mass of H2O = (2x1) + 16 = 18g/mol
Mole of H2O = 9 moles
Mass of H2O =..?
Mole = mass / molar mass
9 = mass of H2O /18
Cross multiply
Mass of H2O = 9 x 18
Mass of H2O = 162g
Therefore, 162g of H2O were produced from 3 moles of C2H6.
