<span>Heat capacity of an object, is the amount of heat energy or thermal energy (unit: Joule) needed to raise the temperature of the object by 1 degree celsius. Unit of heat capacity is J/°C
Larger object will surely need larger amount of thermal energy to raise its temperature. If you compare 1 litre of water with 0.5 litre of water, the 1L water will have two times the heat capacity.
It will be more useful to compare specific heat capacity, because then it is the amount of heat energy or thermal energy (unit: Joule) needed to raise the temperature of 1 unit mass of the object by 1 degree celsius. You can then compare between 1 unit mass of water and 1 unit mass of iron.
Water has higher specific heat capacity than iron, meaning that you need more energy to heat up 1kg of water, then to heat up 1kg of iron.
The unit will then be J/(kg °C) or J/(g °C).
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Answer:
a variable (often denoted by y) whose value depends of that of another.
Explanation:
on g00gle duhh just look it up. :)
Answer:
0.0559 mol
Explanation:
Step 1: Given and required data
- Volume of air (V): 1.35 L
- Pressure of air (P): 750 torr
- Ideal gas constant (R): 0.0821 atm.L/mol.K
Step 2: Convert "P" to atm
We will use the conversion factor 1 atm = 760 torr.
750 torr × 1 atm/760 torr = 0.987 atm
Step 3: Convert "T" to Kelvin
We will use the following expression.
K = °C + 273.15
K = 17.0 °C + 273.15 = 290.2 K
Step 4: Calculate the number of moles of air
If we assume air behaves as an ideal gas, we can calculate the moles (n) of air using the ideal gas equation.
P × V = n × R × T
n = P × V/R × T
n = 0.987 atm × 1.35 L/(0.0821 atm.L/mol.K) × 290.2 K = 0.0559 mol
The answer is No. That is the mass of the sealed jar and its contents does not change upon the vaporization of the liquid, as according to the “law of conservation of mass” , the mass remain conserved when no matter is escape, the mass will remain constant and here also as the jar is sealed, no matter is escaped thus no mass change will be there.
Answer:
0.138 moles of oxygen are needed to combine with 0.276 moles of carbon.
Explanation:
Given data:
Moles of oxygen needed = ?
Moles of carbon present = 0.276 mol
Solution:
Chemical equation:
2C + O₂ → 2CO
Now we will compare the moles of carbon with oxygen.
C : O₂
2 : 1
0.276 : 1/2×0.276 = 0.138 mol
Thus, 0.138 moles of oxygen are needed to combine with 0.276 moles of carbon.
