Mass is the property of a physical body and the resistance to acceleration when a net force is applied on the body.
The atomic mass of sodium (Na) is = 22.98
The atomic mass of nitrate (N) is = 14.00
The atomic mass of oxygen (O) is = 15.99
The sodium nitrate (NaNO3) consists of the atomic masses of Na+N+(O)3 = 85 grams
Therefore, the mass of 6.5 mol of sodium nitrate is = 6.5 * 1 mol of NaNO3
= 6.5 * (85)
= 552.50 grams
Explanation:
Since HF is a weak acid, the use of an ICE table is required to find the pH. The question gives us the concentration of the HF.
HF+H2O⇌H3O++F−HF+H2O⇌H3O++F−
Initial0.3 M-0 M0 MChange- X-+ X+XEquilibrium0.3 - X-X MX M
Writing the information from the ICE Table in Equation form yields
6.6×10−4=x20.3−x6.6×10−4=x20.3−x
Manipulating the equation to get everything on one side yields
0=x2+6.6×10−4x−1.98×10−40=x2+6.6×10−4x−1.98×10−4
Now this information is plugged into the quadratic formula to give
x=−6.6×10−4±(6.6×10−4)2−4(1)(−1.98×10−4)−−−−−−−−−−−−−−−−−−−−−−−−−−−−√2x=−6.6×10−4±(6.6×10−4)2−4(1)(−1.98×10−4)2
The quadratic formula yields that x=0.013745 and x=-0.014405
However we can rule out x=-0.014405 because there cannot be negative concentrations. Therefore to get the pH we plug the concentration of H3O+ into the equation pH=-log(0.013745) and get pH=1.86
First, we will get the average pH of the two given values:
average pH = (6.4+8) / (2) = 7.2
At this average pH, the concentration of the acid from the phenol red is equal to the concentration of the base.
pH = 7.2
[H+] = 10^(-7.2) = 6.3 * 10^-8
Phenol red has the general formula HA, this gives us:
HA <.......> H+ + A-
At pH = 7.2, [H+] = [A-]
<span>Ka = [H+][A-]/ [HA]
</span>Ka = [H+] = <span>6.3 x 10^-8</span>
Answer:
relationship between four fundamental physical properties of gases: pressure PP, volume VV, number of moles nn, and the absolute temperature TT. The ideal gas constant is denoted by RR and its exact value depends on the units chosen for the other parameters. Note that the temperature is always in Kelvins (i.e., we use the absolute temperature). The relation is:
PV=nRT
Answer: 0.0944 gram of H2
Explanation:
Raising the T from 25 C (298 K) to 700 C (973 K) increases the pressure of each gas by:
2.0 atm x (973 K / 298 K) = 6.53 atm
Where
Kc = Kp because the moles of product equals the moles of reactants.
At equilibriuim, the amounts are
P(H2) = 6.53 - x
P(CO2) = 6.53 - x
P(H2O) = x
P(CO) = x
Kc = Kp = .534 = (x)(x) / [(6.53 - x)(6.53 - x)]
Take the square root of each side
(.534)^0.5 = x / (6.53 - x)
x = 0.731 (6.53 - x)
x = 4.77 - 0.731x
1.731x = 4.77
x = 4.77 / 1.731 = 2.76 atm
P(H2) at equilibriuim = 6.53 - 2.76 = 3.77 atm
P(CO2) at equilibrium = 6.53 - 2.76 = 3.77 atm
PV = nRT
n = PV/RT = [(3.77 atm)(1.00 L)] / [(0.08206 L atm/K mol)(973 K)] = 0.0472 mol H2
0.0472 mol H2 x (2.00 g / 1.00 mol) = 0.0944 g
