Finally, how does carbon monoxide disrupt the process of oxygen transport? The oxygen diffuses in alveoli through capillaries and goes into the arterial blood. The waste-rich blood from veins, containing carbon dioxide releases carbon dioxide into alveoli. The carbon dioxide follows the same path out of the lungs. The diaphragm is essential for the gas exchange process.
An increase in hydrogen ion concentration would You correctly answered: d. decrease pH. 3. The amount of carbon dioxide in the blood is measured in You correctly answered: b. mm Hg. 4. The reaction of water and carbon dioxide is catalyzed by You correctly answered: a. carbonic anhydrase.
: V (6.0) Pressure ((4.18) *Raised back up to 398.: V (6.0) Pressure (5.51) -Temp. : 349 V (6) P (4.85) -Temp 145 V (6) P (2 point 06) -361 V 6 P 4. 9 -528 P 7.29 -102 P 1.45 -318 P 4.38 -565 P 7.86 -188 P 2.58 -460 P 6.35 -77 P 1.09 IDEAL GAS LAW 1) What is the relationship between pressure and temperature at constant volume? At a constant volume, as the temperature increases, the pressure also increases. 2) Using this data, predict at what temperature the pressure will exceed 10 units If the pressure is 10.1 units, the temperature would be around 732 ° .
A. .0146% B. 146% C. 14.6% D. 1.46% 17. The sum of 1/6, 2/3, and 1/4 is A. 2/72, or 1/36.
Show all work and label the two half-reactions by placing LEO and GER above the appropriate arrows: Answer the following questions that pertain to the reaction above and mark your answers on the Scantron ticket (questions 28 – 37): 28. Which element was reduced in the reaction above? A) S B) Cl C) O D) H 29. Which element was oxidized in the reaction above? A) S B) Cl C) O D) H 30.
(2 points) Mg(s) + 2 HCl(aq) → H2(g) + MgCl2(aq) 2. Determine the partial pressure of the hydrogen gas collected in the gas collection tube. (3 points) partial pressure H2 = total pressure - vapor pressure of water = 746mmHg - 19.8mmHg = 726mmHg 3. Calculate the moles of hydrogen gas collected. (4 points) n = 125 4.
a) for a we first need to find a balanced equation for when the hydrocarbons combust to form CO2 and H20. Then we plug in the deltaHf values and plug these into the equation. a) C4H6 + 11/2O2 ==> 4CO2 + 3H2O Delta Hrxn = [4DeltaHf(CO2)+3DeltaHf(H2O)] - [DeltaHf(C4H6) + 11/2DeltaHf(O2)] = [4(-393.5kJ) + 3(-285.83kJ)] - [111.9kJ + 11/2(0kJ)] = -2543.39kJ C4H8 + 6O2 ==> 4CO2 + 4H2O Delta H rxn = [4DeltaHf(CO2) + 4DeltaHf(H2O)] - [DeltaHf(C4H8) + 6DeltaHf(O2)] = [4(-393.5kJ) + 4(-285.83kJ)] - [1.2kJ +6(0kJ)] = -2718.52kJ C4H10 +13/2O2 ==> 4CO2 +5H2O DeltaHrxn = [4DeltaHf(CO2) + 5DeltaHf(H2O)] - [DeltaHf(C4H10) + 13/2DeltaHf(O2)] = [4(-393.5kJ) + 5(-285.83kJ)] - [-124.7kJ +
As the number of moles decreases, the volume decreases Summary: Combined Gas Law: PV/nT = constant (T in Kelvins) P1V1/n1T1 = P2V2/n2T2 Ideal gas Law: PV = nRT R = .0821L atm/mol K Gay-Lussac’s/Avogadro’s Law of Combining Volumes Equal volumes of any gases at the same temperature and pressure contain the same number of moles of gas. The coefficients of a balanced equation can be used to calculate relative volumes. Standard Molar Volume: At standard temperature and pressure (STP = 1atm and 273.15K) 1 mole of any ideal gas has a volume of 22.4L Variations on the ideal gas law equation: PV = mRT/M (m = sample mass, M = molar mass of the gas) d = MP/RT (d = density of the gas in g/L) Examples: 1. Calculate: a. The new pressure in a closed container if a 5.0L volume of gas at 2.5atm has its volume increased to 7.5L.
Once the wavelength is calculated, the heat capacity ratio for each of the gases will be calculated. Introduction When temperature is increased in a system, the internal energy is raised. It is assumed that the system has a constant volume, so the increase depends on different conditions based on which the heating takes place. If internal energy is plotted against temperature, a curve can be seen in a graph. The graph shows a variation as the system heats at a constant volume.
59. Fill in the missing particle or element from the periodic table for X. Indicate mass and charge. a) 60Co ( X + 60Ni 27 28 b) 231Th ( X + 0 e 90 -1 c) X ( 20Ne + 0 e 10 -1 60. Phosphorus–32, has a half-life of 14 days.