Water can dissolve salt because the positive part of water molecules attracts the negative chloride ions and the negative part of water molecules attracts the positive sodium ions. The amount of a substance that can dissolve in a liquid (at a particular temperature) is called the solubility of the substance.
I think the correct answer would be the third option. An example of a pure research would be creating synthetic elements to study their properties. Pure research is also known as fundamental or basic research. It has an exploratory nature wherein it is done without any end use in mind. It is mostly out of the curiosity or intuition of a researcher. Most of the study under this type is aiming to advance an existing knowledge by explaining or identifying the relationship of the variables being studied. It is aimed at improving theories in order to the understanding of a specific phenomenon.
Answer:
<h3>The answer is 0.67 cm³ </h3>
Explanation:
Density of a substance can be found by using the formula
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</h3>
Making volume the subject we have
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</h3>
From the question
mass of gold nugget = 13 g
Density = 19.3 g/cm³
Substitute the values into the above formula and solve for the volume
We have
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</h3>
= 0.673575
We have the final answer as
<h2>0.67 cm³</h2>
Hope this helps you
Yes sir I’m not sure why what I said so yes sir I’m not gonna go to the bathroom I’m just gonna go home I’m gonna be there in about a week or two I don’t uueiueyey
Hydrogen gas and oxygen gas react to form liquid water according to the following equation:
2H₂ + O₂ → 2H₂O
a. Converting our given masses of each gas to moles, we have:
(25 g H2)/(2 × 1.008 g/mol) = 12.4 mol H2; and
(25 g O2)/(2 × 15.999 g/mol) = 0.781 mol O2.
From the equation, two moles of H2 react with every one mole of O2. To fully react with 12.4 moles of H2, as we have here, one would need 6.2 moles of O2, which is far more than what we're actually given. Thus, the oxygen is our limiting reactant, and as such it will be the first reactant to run out.
b. Since O2 is our limiting reactant, we use it for determining how much product, in this case, H2O, is produced. From the equation, there is a 1:1 molar ratio between O2 and H2O. Thus, the number of moles of H2O produced will be the same as the number of moles of O2 that react: 0.781 moles of H2O. The mass of water produced would be (0.781 mol H2O)(18.015 g/mol) ≈ 14 grams of water (the answer is given to two significant figures).
c. Since the hydrogen reacts with the oxygen in a 2:1 ratio, twice the number of moles of oxygen in hydrogen is consumed: 0.781 mol O2 × 2 = 1.562 mol H2. Since we began with 12.4 moles of H2, the remaining amount of excess H2 would be 12.4 - 1.562 = 10.838 mol H2. The mass of the excess hydrogen reactant would thus be (10.838 mol H2)(2 × 1.008 g/mol) ≈ 22 grams of hydrogen gas (the answer is given to two significant figures).
