Answer:
the volume occupied by 3.0 g of the gas is 16.8 L.
Explanation:
Given;
initial reacting mass of the helium gas, m₁ = 4.0 g
volume occupied by the helium gas, V = 22.4 L
pressure of the gas, P = 1 .0 atm
temperature of the gas, T = 0⁰C = 273 K
atomic mass of helium gas, M = 4.0 g/mol
initial number of moles of the gas is calculated as follows;
The number of moles of the gas when the reacting mass is 3.0 g;
m₂ = 3.0 g
The volume of the gas at 0.75 mol is determined using ideal gas law;
PV = nRT
Therefore, the volume occupied by 3.0 g of the gas is 16.8 L.
Answer:
C) It moves faster and collects more data
Explanation:
It either forms a base or an acid...I think that's the answer you're looking for
Answer:
Approximately .
Explanation:
Balanced equation for this reaction:
.
Look up the relative atomic mass of elements in the limiting reactant, , as well as those in the product of interest, :
Calculate the formula mass for both the limiting reactant and the product of interest:
.
.
Calculate the quantity of the limiting reactant () available to this reaction:
.
Refer to the balanced equation for this reaction. The coefficients of the limiting reactant () and the product () are both . Thus:
.
In other words, for every of formula units that are consumed, of formula units would (in theory) be produced. Thus, calculate the theoretical yield of in this experiment:
.
Calculate the theoretical yield of this experiment in terms of the mass of expected to be produced:
.
Given that the actual yield in this question (in terms of the mass of ) is , calculate the percentage yield of this experiment:
.
Monoprotic acid are acids having
only one hydrogen atoms after dissociation into ions from its compound. The
monoprotic acid from among the following is HCl. The answer is letter D. HCl →
H+ + Cl-. Note that there is only one H+ ion upon dissociation.