I'm not 100% sure on this, but I would go with C) NaCl.
NaCl is a salt, and that is used to melt the ice on the roads. Hope this helps!
Answer:
Explanation:
Hermione is pretty smart. She realizes that, according to Dalton's Law of Partial Pressures, each gas exerts its pressure independently of the others, as if the others weren't even there.
She shows Ron how to use the Ideal Gas Law to solve the problem.
pV = nRT
She collects the data:
V = 1.00 L; n = 0.0319 mol; T = 25.0 °C
She reminds him to convert the temperature to kelvins
T = (25.0 +273.15) K = 298.15 K
Then she shows him how to do the calculation.
Isn't she smart?
When we can get the Kinetic energy from this formula KE= 1/2 M V^2and we can get the potential energy from this formula PE = M g H
we can set that the kinetic energy at the bottom of the fall equals the potential energy at the top so, KE = PE
1/2 MV^2 = M g H
1/2 V^2 = g H
when V is the velocity, g is an acceleration of gravitational force (9.8 m^2/s) and H is the height of the fall (8 m).
∴ v^2 = 2 * 9.8 * 8 = 156.8
∴ v= √156.8 = 12.5 m/s
Answer: V= 3.13 L
Explanation: solution attached:
Use combine gas law equation:
P1 V1 / T1 = P2 V2/ T2
Derive to find V2
V2 = P1 V1 T2 / T1 P2
Convert temperatures in K
T1= 13.0°C + 273 = 286 K
T2= 22.5°C + 273 = 295.5 K
Substitute the values.
Answer:
a. both temperature changes will be the same
Explanation:
When sodium hydroxide (NaOH) is dissolved in water, a determined amount is released to the solution following the equation:
Q = m×C×ΔT
<em>Where Q is the heat released, m is the mass of the solution, C is the specific heat and ΔH is change in temperature.</em>
Specific heat of both solutions is the same (Because the solutions are in fact the same). Specific heat = C.
m is mass of solutions: 102g for experiment 1 and 204g for experiment 2.
And Q is the heat released: If 2g release X heat, 4g release 2X.
Thus, ΔT in the experiments is:
Experiment 1:
X / 102C = ΔT
Experiment 2:
2X / 204C = ΔT
X / 102C = ΔT
That means,
<h3>a. both temperature changes will be the same</h3>
