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As the temperature of a liquid increases, its viscosity decreases.
Answer:
Final temperature of the mixture is 50°C
Explanation:
This is a typical calorimetry problem, where the heat yielded by a compound is immediately won by another.
Water at 90°C raise the temperature of water at 10°
Density of water = 1g/mL
Mass of water = 100 g, because the volume is 100mL
If the two pieces of water are in a calorimeter where heat is not released or gained, the sum of both heats is 0
4.18 J/g°C . 100 g ( T°final - 90°C) + 4.18 J/g°C . 100 g ( T°final - 10°C) = 0
418 J/°C T°final - 37620 J + 418 J/°C T°final - 4180J = 0
836 J/°C T°final - 37620J - 4180J = 0
836 J/°C T°final = 41800J
T°final = 41800J / 836 °C/J = 50°C
Answer is: V has the units of liters, and T has the units of kelvin.
Ideal gas law: p·V = n·R·T.
atm · L = mol · L·atm/mol·K · K; both side of equatation have same values.
R = 0,08206 L·atm/mol·K; universal gas constant.
p is pressure of the gas, unit is standard atmosphere (atm).
V is volume of the gas, unit is liters (L).
n is amount of substance of the gas; unit is mole (mol).
T is temperature of the gas, unit is Kelvin (K).