Answer:- 13.6 L
Solution:- Volume of hydrogen gas at 58.7 Kpa is given as 23.5 L. It asks to calculate the volume of hydrogen gas at STP that is standard temperature and pressure. Since the problem does not talk about the original temperature so we would assume the constant temperature. So, it is Boyle's law.
Standard pressure is 1 atm that is 101.325 Kpa.
Boyle's law equation is:
From given information:-
= 58.7 Kpa
= 23.5 L
= 101.325 Kpa
= ?
Let's plug in the values and solve it for final volume.
On rearranging the equation for
= 13.6 L
So, the volume of hydrogen gas at STP for the given information is 13.6 L.
Answer:
C) Modernization of humans
Answer:
The mass of the products left in the test tube will be less than that of the original reactants.
Explanation
The equation for the reaction is
Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
1.0 3.0 3.9 0.1
Assume you started with 1.0 g of Mg.
It will react with 3.0 g of HCl to form 3.9 g of MgCl2 and 0.1 g of H2
.
Mass of reactants = mass of products
1.0 g + 3.0 g = 3.9 g + 0.1 g
4.0 g = 4.0 g
The Law of Conservation of Mass is obeyed.
However, your test tube and its contents will weigh 0.1 g less than it did before the reaction.
Does that contradict the Law of Conservation of Mass? It does not.
One of the products was the gas, hydrogen, and it escaped from the test tube. You weren't measuring all the products, so test tube and its contents weighed less than before.
The mass of NiCl₂•6HO₂ needed to prepare a 0.035 M 500 mL solution of NiCl₂•6HO₂ is 4.165 g
<h3>What is molarity? </h3>
This is defined as the mole of solute per unit litre of solution. Mathematically, it can be expressed as:
Molarity = mole / Volume
<h3>How to determine the mole of NiCl₂•6HO₂</h3>
- Molarity = 0.035 M
- Volume = 500 mL = 500 / 1000 = 0.5 L
Mole = Molarity × Volume
Mole of NiCl₂•6HO₂ = 0.035 × 0.5
Mole of NiCl₂•6HO₂ = 0.0175 mole
<h3>How to determine the mass of NiCl₂•6HO₂</h3>
- Mole of NiCl₂•6HO₂ = 0.0175 mole
- Molar mass of NiCl₂•6HO₂ = 238 g/mol
Mass = mole × molar mass
Mass of NiCl₂•6HO₂ = 0.0175 × 238
Mass of NiCl₂•6HO₂ = 4.165 g
Thus, 4.165 g of NiCl₂•6HO₂ is needed to prepare the solution
Learn more about molarity:
brainly.com/question/15370276
