Answer:
D. The rate decreases as reactants are used up.
Explanation:
Initially, the rate increases until the reaction is at equilibrium. At equilibrium, the rate is constant.
As the reaction progresses, the rate decreases to zero when reactants are used up ( for irriversible reactions only )
Using natural gas is cheaper from other fossil fuels when used for personal needs. It also doesn't pollute the ground or the underground water.
Answer:
Photosynthetic bacteria must take in <u>Carbon Dioxide</u> to live, and they release <u>Oxygen </u> . Animals must take <u>Oxygen </u> to live, and they release <u>Carbon Dioxide.</u>
Explanation:
Photosynthesis:
It is the process in which in the presence of sun light and chlorophyll by using carbon dioxide and water plants produce the oxygen and glucose.
Carbon dioxide + water + energy → glucose + oxygen
water is supplied through the roots, carbon dioxide collected through stomata and sun light is capture by chloroplast.
Chemical equation:
6H₂O + 6CO₂ + energy → C₆H₁₂O₆ + 6O₂
Photosynthetic bacteria perform same function as plants. These bacteria contain light harvesting pigments absorb carbon dioxide and release oxygen.
While animals take oxygen and release carbon dioxide to live. This respiration process is opposite to the photosynthesis.
Glucose + oxygen → carbon dioxide + water + 38ATP
Answer:
ΔH vaporization of chloroform is 30.1kJ/mol
Explanation:
It is possible to find ΔH of vaporization of certain compound knowing vapor pressure under 2 different absolute temperatures (In Kelvin) by using Clausius-Clapeyron equation:
![ln\frac{P_2}{P_1}=\frac{DeltaHvap}{R} (\frac{1}{T_1} - \frac{1}{T_2} )](https://tex.z-dn.net/?f=ln%5Cfrac%7BP_2%7D%7BP_1%7D%3D%5Cfrac%7BDeltaHvap%7D%7BR%7D%20%20%28%5Cfrac%7B1%7D%7BT_1%7D%20-%20%5Cfrac%7B1%7D%7BT_2%7D%20%29)
<em>Where P is vapor pressure. R is gas constant (8.314J/molK) and T absolute temperature of 1, first state and 2, final state.</em>
Absolute temperatures in the problem are:
T₁ = 24.1°C + 273.15 = 297.25K
T₂ = -6.3°C + 273.15 = 266.85K
Replacing:
![ln\frac{P_2}{P_1}=\frac{DeltaHvap}{R} (\frac{1}{T_1} - \frac{1}{T_2} )](https://tex.z-dn.net/?f=ln%5Cfrac%7BP_2%7D%7BP_1%7D%3D%5Cfrac%7BDeltaHvap%7D%7BR%7D%20%20%28%5Cfrac%7B1%7D%7BT_1%7D%20-%20%5Cfrac%7B1%7D%7BT_2%7D%20%29)
![ln\frac{100torr}{400.0torr}=\frac{DeltaHvap}{8.314J/molK} (\frac{1}{297.25K} - \frac{1}{266.85K} )](https://tex.z-dn.net/?f=ln%5Cfrac%7B100torr%7D%7B400.0torr%7D%3D%5Cfrac%7BDeltaHvap%7D%7B8.314J%2FmolK%7D%20%20%28%5Cfrac%7B1%7D%7B297.25K%7D%20-%20%5Cfrac%7B1%7D%7B266.85K%7D%20%29)
![ln\frac{100torr}{400.0torr}={DeltaHvap}* -4.6x10^{-5}mol/J](https://tex.z-dn.net/?f=ln%5Cfrac%7B100torr%7D%7B400.0torr%7D%3D%7BDeltaHvap%7D%2A%20-4.6x10%5E%7B-5%7Dmol%2FJ)
30073J/mol = 30.1kJ/mol = ΔHVap
<h3>ΔH vaporization of chloroform is 30.1kJ/mol</h3>