Answer:
T = 377.2 K, Less than
Explanation:
The thermodynamic quantity used in predicting whether a reaction is spontaneous or not is the gibbs free energy.
It's relationship with ΔH⁰ and ΔS⁰ is given as;
ΔG° = ΔH° - TΔS°
Basically, a negative value of ΔG° means the reaction is spontaeneous.
To obtain the calculated vale of T,
ΔS° = ΔH°/T
T = ΔH° / ΔS°
T = 377.2 K
Let's calculate the value of ΔG° at that temperature.
ΔG° = ΔH° - TΔS°
ΔG° = − 46700 - 377.2(− 123.8)
ΔG° = 0 (approximately, values are due to the rounding off)
At ΔG° = 0 the reaction is at equilibrium.
To find if the reaction is spontaneous at lower or hugher temperature than the calculated temperature, we would be substituting the value of T with a smaller (random) value and also a larger (random) value.
Larger T (390K)
ΔG° = ΔH° - TΔS°
ΔG° = − 46700 - 390(− 123.8)
ΔG° = - 46700 + 48,282
ΔG° = 1582 J/mol
Smaller T (350K)
ΔG° = ΔH° - TΔS°
ΔG° = − 46700 - 350(− 123.8)
ΔG° = - 46700 + 43330
ΔG° = -3370J/mol
This means the temperature would be lesser than the calculated value for it to be spontaneus.
The answer is 4 Newton
force = mass x acceleration
F= 2 kg x 2.0 <span>m<span>s2</span></span>
= 4 Newton
Answer:
THE HEAT OF COMBUSTION IS 4995.69 kJ/mol OF OCTANE.
Explanation:
Heat capacity = 6.18 kJ/C
Temperature change = 41.5 C - 22.0 C = 19.5 C
Heat required to raise the temperature by 19.5 °C is:
Heat = heat capacity * temperature change
Heat = 6.18 kJ/ C * 19.5 C
heat = 120.51 kJ of heat
120.51 kJ of heat is required to raise the temperature of 2.75 g sample of a liquid octane.
Molar mass of octane = ( 12* 8 + 1 * 18) = 114 g/mol
So therefore, the heat of the reaction per mole of octane will be:
120.51 kJ of heat is required for 2.75 g of octane
x J of heat will be required for 114 g of octane
x J = 120.51kJ * 114 / 2.75
x = 4995.69 kJ of heat per mole.
In conclusion, the heat of the combustion reaction in kJ / mole of octane is 4995.69 kJ/mol
Answer:
The solid will start to transition from a solid to a liquid.
Explanation:
When a solid reaches the point of its melting point, the substance will start to turn into liquid form. As long as energy is constantly added, it will soon turn fully liquid. However, when it reaches it melting point, it will flip back and forth from solid to liquid form (solid to liquid equilibrium) until the energy added allows it to become fully liquid.
Take H2O for example. The melting point of solid water is 0°C. At that point, the solid ice starts to turn into water, but still is kinda solid and the ice shape is still there. When it is continuously heated (add energy), it will turn into liquid H2O.
