Answer:
When two substances having different temperatures are introduced or kept together, heat energy, Q, flows from a substance at higher temperature to a substance at lower temperature. Also, heat continues to be transferred until their temperatures are equalized, at which point the substances are in thermal equilibrium. In a closed system, the amount of energy lost is equal to but opposite the amount of energy gained.
Explanation:
Answer:
378.25°C
Explanation:
Given data:
Number of moles of gas = 0.750 mol
Volume of gas = 35.9 L
Pressure of gas = 114 KPa (114/101 = 1.125 atm)
Temperature of gas = ?
Solution:
The given problem will be solve by using general gas equation,
PV = nRT
P= Pressure
V = volume
n = number of moles
R = general gas constant = 0.0821 atm.L/ mol.K
T = temperature in kelvin
now we will put the values.
T = PV/nR
T = 1.125 atm × 35.9 L /0.750 mol × 0.0821 atm.L/ mol.K
T = 40.3875/0.062/K
T = 651.4 K
Kelvin to °C:
651.4 K - 273.15 = 378.25°C
Answer:
The concentration of 
is 1.48 × 
M
The absolute uncertainty of ![[{H^{+}]](https://tex.z-dn.net/?f=%5B%7BH%5E%7B%2B%7D%5D)
is ±0.12 × M
The concentration of is written as 1.48(±0.12) × M
Explanation:
The pH of a solution is given by the formula below
pH = ![-log_{10}[{H^{+}]](https://tex.z-dn.net/?f=-log_%7B10%7D%5B%7BH%5E%7B%2B%7D%5D)
∴ ![[H^{+}] = 10^{-pH}](https://tex.z-dn.net/?f=%5BH%5E%7B%2B%7D%5D%20%3D%2010%5E%7B-pH%7D)
where is the concentration
From the question,
pH = 8.83±0.04
That is,
pH =8.83 and the uncertainty is ±0.04
First, we will determine from
![[{H^{+}] = 10^{-8.83}](https://tex.z-dn.net/?f=%5B%7BH%5E%7B%2B%7D%5D%20%3D%2010%5E%7B-8.83%7D)
![[{H^{+}] = 1.4791](https://tex.z-dn.net/?f=%5B%7BH%5E%7B%2B%7D%5D%20%3D%201.4791)
× M
![[{H^{+}] = 1.48](https://tex.z-dn.net/?f=%5B%7BH%5E%7B%2B%7D%5D%20%3D%201.48)
× M
The concentration of is 1.48 × M
The uncertainty of ( ![U_{[H^{+}] }](https://tex.z-dn.net/?f=U_%7B%5BH%5E%7B%2B%7D%5D%20%7D)
) from the equation is
![U_{[H^{+}] } = 2.303 \\](https://tex.z-dn.net/?f=U_%7B%5BH%5E%7B%2B%7D%5D%20%7D%20%3D%202.303%20%5C%5C)
× ![{[H^{+}] }](https://tex.z-dn.net/?f=%7B%5BH%5E%7B%2B%7D%5D%20%7D)
× 
Where is the uncertainty of
is the uncertainty of the pH
Hence,
= 2.303 × 1.4791 × × 0.04
= 1.36 × 
M
= 0.12 × M
Hence, the absolute uncertainty of is ±0.12 × M
Answer: Conclusion
Explanation:
After they test the hypothesis they come to a conclusion of the answer.
and sometime test it again and again
