Answer:
1.77 g/L.
Explanation:
Molar mass of CO2 = 12 + (16*2)
= 44 g/mol.
Using ideal gas equation,
V/n = R*T/P
Where,
R = 0.082 L.atm/mol.K
T = 30°C
= 273 + 30
= 303 K
P = 1 atm
V/n = (0.082 * 303)/1
= 24.845 L/mol
Density = mass * volume
Density = molar volume/molar mass
= 44/24.845
= 1.77 g/L
It is a good idea because when mercury heats up, the molecules spread farther apart. Therefore, making them look to have expanded. Thermometers that are digital use a sensor to, as you would say feel the temperature around it.
Answer:
1. Qsol = -5.87 kJ
2. ΔHrn = 18.4 kJ/mol
Explanation:
According to the law of conservation of energy, the sum of the heat absorbed by the reaction and the heat released by the solution is zero.
Qrn + Qsol = 0
Qrn = -Qsol
We can calculate the heat released by the solution using the following expression.
Qsol = c . m . ΔT
where,
c: specific heat capacity of the solution
m: mass of the solution
ΔT: change in the temperature
Qsol = (4.184 J/g.°C) . (243g + 32.3g) . (17.90°C-23.00°C) = -5.87 × 10³ J = -5.87 kJ
The heat absorbed by the reaction is:
Qrn = -Qsol = 5.87 kJ
In the balanced equation, we have 1 mole of KNO₃. Given we are in a constant-pressure calorimeter, the enthalpy of reaction (per mole of KNO₃) is:
Answer: thermochromism, too hot of temperature or long exposure to high temperature may completely degrade the color of an object. In other instances, an object or sample changes to another shade of color until it stabilizes back to room temperature.
Explanation: