Answer:
m = 65.637 g
Explanation:
Heat = 0.612 kJ = 612 J ( Converting to J by multiplying by 1000)
Initial Temperature = 30.°C
Final Temperature = 51°C
Temperature change = Final Temperature - Initial Temperature = 51 - 30 = 21°C
Mass = ?
The relationship between these quantities is given by the equation;
H = mCΔT
where c = 0.444 J/g°C
Inserting the values in the equation;
612 = m * 0.444 * 21
m = 612 / (0.444 * 21)
m = 65.637 g
Have about 5 beakers all with different temperatures of water. Put in a teaspoon of salt at a time and when it stops dissolving stop adding and record how much salt it took. It should be more salt as the temperature rises. The independent variable is the waters temperature. The dependent variable is how much salt is used. Make sure that there is the same amount of water in each beaker. Or else it won’t work.
Answer:
bruh, just go in your bathroom and look for cleaning products
Explanation:
Answer:
929.4 kJ of heat is released.
Explanation:
The enthalpy of vaporization of hydrogen sulfide is 18.7 kJ/mol at -60.0 °C.
The data explains that 1 mol of H₂S uses 18.7 kJ of energy in vaporization.
By the Ideal Gas Law, we can know, how many moles do we have, of gas.
P. V = n . R . T
87 atm . 10L = n . 0.0821 L.atm/K.mol . 213 K
(87 atm . 10L) / (0.0821 K.mol/L.atm . 213 K) = 49.7 moles
1 mol ____ 18.7 kJ
49.7 moles _____ (49.7 . 18.7) = 929.4 kJ
