The answer to this question will be C
Answer: The temperature of the gas if 65.85g of N2 are placed in 17.5L container with a pressure of 1988 mmHg is 1780. 6° C
Explanation:
The ideal gas law states that the volume, pressure and temperature of the a gas is related to the number of moles.
It is represented thus;
P V = n R T
Parameters :
Pressure, P = 1988 mmHg
Volume, V = 17.5 L
number of moles, n = mass ÷ molar mass
mass of N2 = 65.84g
Molar mass of N2 = 28.02 g/ mol
n = 65.85 ÷ 28.02
n = 2. 350 moles.
Temperature = ?
Universal gas constant, R = 8.314 J/mol. K
Calculations :
T = P V ÷ n R
T = 1988 × 17.5 ÷ 2.350 × 8.314
T = 34790 ÷ 19. 5379
T = 1780. 6 ° C
Thus, the temperature of the gas is 1780. 6 ° C
I hope that you can understand this!!! Lol
The thing that you have to pull back to release with, that would be considered a third class lever.
I hope this helps. :)
Answer:
[NaCH₃COO] = 2.26M
Explanation:
17% by mass is a sort of concentration. Gives the information about grams of solute in 100 g of solution. (In this case, 17 g of NaCH₃COO)
Let's determine the volume of solution, by density
Mass of solution / Volume of solution = Solution density
100 g / Volume of solution = 1.09 g/mL
100 g / 1.09 g/mL = 91.7 mL
17 grams of solute is contained in 91.7 mL
Molarity (M) = Mol of solute /L of solution
91.7 mL / 1000 = 0.0917L
17 g / 82 g/m = 0.207 moles
Molariy = 0.207 moles / 0.0917L → 2.26M