Answer:
Specific heat of metal = 0.26 j/g.°C
Explanation:
Given data:
Mass of sample = 80.0 g
Initial temperature = 55.5 °C
Final temperature = 81.75 °C
Amount of heat absorbed = 540 j
Specific heat of metal = ?
Solution:
Specific heat capacity:
It is the amount of heat required to raise the temperature of one gram of substance by one degree.
Formula:
Q = m.c. ΔT
Q = amount of heat absorbed or released
m = mass of given substance
c = specific heat capacity of substance
ΔT = change in temperature
ΔT = 81.75 °C - 55.5 °C
ΔT = 26.25 °C
540 j = 80 g × c × 26.25 °C
540 j = 2100 g.°C× c
540 j / 2100 g.°C = c
c = 0.26 j/g.°C
Answer:
A medida que aumenta la temperatura de un líquido, la solubilidad de los gases en ese líquido disminuye. Podemos usar la Segunda Ley de la Termodinámica para explicar por qué. Calentar una solución de un gas permite que las partículas de gas se muevan más libremente entre la solución y la fase gaseosa. La Segunda Ley predice que cambiarán al estado más desordenado, más altamente disperso y, por lo tanto, más probablemente gaseoso.
Explanation:
1. <span>The answer should be combustion
2. </span><span>Water is known to successfully dissolve both acids and bases, and water is considered a universal solvent.
3. The answer should be balanced.
Hope this helps :)
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Answer:
Option b. 9.59
Explanation:
First, let us calculate the pH. This is illustrated below:
[H3O+] = 3.9 x 10-5 M
pH = —Log [H3O+]
pH = —Log [3.9 x 10-5]
pH = 4.41
Recall: pH + pOH = 14
4.41 + pOH = 14
Collect like terms
pOH = 14 — 4.41
pOH = 9.59
Answer:
14.61 g NaCl
Explanation:
Molarity = moles / volume of solution (litres)
0.500 = moles / 0.500 L
moles = 0.25
Molar mass of NaCl is 58.44 g NaCl /1 mol NaCl.
0.25 moles NaCl x 58.44 g NaCl /1 mol NaCl
= 14.61 g NaCl
