Answer:
0.33 ml
Explanation:
Formula for density: p = m/V (where p is <em>density</em>, m is <em>mass</em> and V is <em>volume</em>)
So, by applying the above formula:
![19.3 = \frac{6.5}{v}](https://tex.z-dn.net/?f=19.3%20%3D%20%20%5Cfrac%7B6.5%7D%7Bv%7D%20)
![v = 0.33 \: ml](https://tex.z-dn.net/?f=v%20%3D%200.33%20%5C%3A%20ml)
133.0873 g/mol
(NH4)3PO3 - molar mass
Answer:
W = -262 J.
Explanation:
Hello there!
In this case, according to the given information, we can recall the definition of work in terms of constant pressure and variable volume as follows:
![W=P(V_2-V_1)](https://tex.z-dn.net/?f=W%3DP%28V_2-V_1%29)
So we plug in the given pressure and volumes to obtain:
![W=0.822atm(1.20L-4.35L)\\\\W=-2.60atm*L](https://tex.z-dn.net/?f=W%3D0.822atm%281.20L-4.35L%29%5C%5C%5C%5CW%3D-2.60atm%2AL)
Now, we convert this number to J (Pa*m³) by using the shown below conversion factor:
![W=-2.60atm*L*\frac{101325Pa}{1atm} *\frac{1m^3}{1000L}\\\\W=-262J](https://tex.z-dn.net/?f=W%3D-2.60atm%2AL%2A%5Cfrac%7B101325Pa%7D%7B1atm%7D%20%2A%5Cfrac%7B1m%5E3%7D%7B1000L%7D%5C%5C%5C%5CW%3D-262J)
Regards!
Answer:
![Cl_2+2NaI\rightarrow I_2+2NaCl](https://tex.z-dn.net/?f=Cl_2%2B2NaI%5Crightarrow%20I_2%2B2NaCl)
Explanation:
Hello there!
In this case, according to the described chemical reaction, Cl2 replaces iodine in NaI in order to produce I2 and NaCl:
![Cl_2+NaI\rightarrow I_2+NaCl](https://tex.z-dn.net/?f=Cl_2%2BNaI%5Crightarrow%20I_2%2BNaCl)
It is possible to realize how chlorine replaces iodine in agreement with the single displacement reaction. Moreover, since chlorine and iodine atoms are not correctly balanced, we add a 2 in front of both NaI and NaCl in order to do so:
![Cl_2+2NaI\rightarrow I_2+2NaCl](https://tex.z-dn.net/?f=Cl_2%2B2NaI%5Crightarrow%20I_2%2B2NaCl)
Best regards!
Answer:
<em>At equilibrium, the rate of the forward, and the reverse reactions are equal.</em>
Explanation:
In an equilibrium chemical reaction, the rate of forward reaction, is equal to the rate of reverse reaction. Note that the reactions does not cease at equilibrium, but rather, the reactants are converted to product, at the same rate at which the product is also being converted into the reactants in the reaction. When chemical equilibrium is reached, a careful calculation of the value of equilibrium constant is approximately equal to 1.
NB: If the value of equilibrium constant is far far greater than 1, then the reaction will favors more of the forward reaction, and if far far less than 1, the reaction will favor more of the reverse reaction.