Ammonia is the most basic and has the highest OH- concentration since it has the highest pH.
Answer:
Partial pressure of oxygen = 23.38 kpa (Approx)
Explanation:
Given:
Amount of oxygen = 23.15%
Amount of nitrogen = 76.85%
Pressure (missing) = 101 kpa
Find:
Partial pressure of oxygen
Computation:
Partial pressure of oxygen = [Amount of oxygen x Pressure]/100
Partial pressure of oxygen = [23.15% x 101]/100
Partial pressure of oxygen = 23.38 kpa (Approx)
Explanation:
A chemical equilibrium is defined as the state of reaction in which the rate of forward reaction is equal to the rate of backward reaction.
When Q > 
, then it means that the reaction is proceeding in the backward reaction. Whereas if Q < , then it means that the reaction is proceeding in the forward direction. Hence, formation of products will be favored.
On the other hand, if Q = , then it means reaction is at equilibrium.
At equilibrium, it is not necessary that the concentrations of products divided by the concentrations of reactants equals one.
Thus, we can conclude that the statement for a chemical system at equilibrium, the forward and reverse rates of reaction are equal, is correct.
Answer:
123.2 Liters.
Explanation:
At STP (T = 273K & P = 1atm)<em>, one mol of any gas will occupy 22.4 liters</em>.
With the above information in mind, we can <u>calculate how many liters would 5.500 mol of gas occupy</u>:
5.500 mol * 22.4 L / mol = 123.2 L
So 5.500 moles of C₃H₃ would have a volume of 123.2 liters at STP.
Answer:
10.56 g
Explanation:
C4H10(g) + 13/2O2 (g) -------> 4CO2(g) + 5H2O(l)
Number of moles of butane = 3.49g/ 58 g/mol = 0.06 moles
1 mole butane yields 4 moles of CO2
0.06 moles of butane = 0.06 × 4/1 = 0.24 moles of CO2
Number of moles of oxygen = 17.1g/32g/mol = 0.53 moles of oxygen
6.5 moles of oxygen yields 4 moles of CO2
0.53 moles of oxygen yields 0.53 × 4/6.5 =0.33 moles of CO2
Butane is the limiting reactant
Theoretical yield of CO2 = 0.24 moles × 44g/mol = 10.56 g
