Answer:
ΔG = -105.4 kJ/mol
The system is spontaneous as written.
Explanation:
Step 1: Determine Gibbs free energy of reaction (ΔG)
We use the following expression.
ΔG = ΔH - T × ΔS
where,
ΔG = ΔH - T × ΔS
ΔG = 120.5 kJ/mol - 298 K × 0.7582 kJ/mol.K
ΔG = -105.4 kJ/mol
Step 2: Determine the spontaneity of the system.
Since ΔG < 0, the system is spontaneous as written.
Answer:
Q = 197505J
Explanation:
Mass (m) = 825g
Specific heat capacity (c) = 1.8J/g°C
Initial temperature (T1) = 22°C
Final temperature (T2) = 155°C
Heat energy (Q) = ?
Q = mc∇t
Q = mc(T2 - T1)
Q = 825 * 1.8 * (155 - 22)
Q = 1485 * 133
Q = 197505J
The heat energy required to raise it through that temperature is 197505J
Answer:
Volume of NaOH reacted = 1.6 L
Explanation:
<u>Given:</u>
Molarity of H2SO4, M1 = 4.0 M
Volume of H2SO4, V1 = 0.6 L
Molarity of NaOH, M2 = 3.0 M
<u>To determine:</u>
Volume of NaOH,V2
<u>Explanation:</u>
The given neutralization reaction is:
Here 2 moles of NaOH reacts with 1 mole of H2SO4
i.e. moles of NaOH = 2(moles of H2SO4)
Since:
Answer:
The easiest way to separate a mixture of sugar and water is to use distillation, a process that separates substances based on their different boiling points.
hope this helps