Answer:
12 moles of propane.
Explanation:
From the question given above, the following data were obtained:
Volume (V) = 216 L
Pressure (P) = 184.8 KPa
Temperature (T) = 127 °C
Number of mole (n) =?
Next, we shall convert 127 °C to Kelvin temperature. This can be obtained as follow:
T(K) = T(°C) + 273
T(°C) = 127 °C
T(K) = 127 + 273
T(K) = 400 K
Finally, we shall determine the number of mole of propane gas in the container. This can be obtained as follow:
Volume (V) = 216 L
Pressure (P) = 184.8 KPa
Temperature (T) = 400 K
Gas constant (R) = 8.314 L.KPa/Kmol
Number of mole (n) =?
PV = nRT
184.8 × 216 = n × 8.314 × 400
39916.8 = n × 3325.6
Divide both side by 3325.6
n = 39916.8 / 3325.6
n = 12 moles
Thus, 12 moles of propane is present in the cylinder
Answer: First, here is the balanced reaction: 2C4H10 + 13O2 ===> 8CO2 + 10H2O.
This says for every mole of butane burned 4 moles of CO2 are produced, in other words a 2:1 ratio.
Next, let's determine how many moles of butane are burned. This is obtained by
5.50 g / 58.1 g/mole = 0.0947 moles butane. As CO2 is produced in a 2:1 ratio, the # moles of CO2 produced is 2 x 0.0947 = 0.1894 moles CO2.
Now we need to figure out the volume. This depends on the temperature and pressure of the CO2 which is not given, so we will assume standard conditions: 273 K and 1 atmosphere.
We now use the ideal gas law PV = nRT, or V =nRT/P, where n is the # of moles of CO2, T the absolute temperature, R the gas constant (0.082 L-atm/mole degree), and P the pressure in atmospheres ( 1 atm).
V = 0.1894 x 0.082 x 273.0 / 1 = 4.24 Liters.
Explanation:
Answer:
Answer down below
Explanation:
if it has to be 2 of these I think it would be A and B but if it is only one Answer it would be B
Answer:
hope this helps
Explanation:
glycosidic bond
A covalent bond formed between a carbohydrate molecule and another molecule (in this case, between two monosaccharides) is known as a glycosidic bond (Figure 4). Glycosidic bonds (also called glycosidic linkages) can be of the alpha or the beta type.
No, Heat moves from concentrations of high to low.
