Geiger–Marsden experiment(s)<span> (also called the </span>Rutherford gold foil experiment<span>) were a landmark series of experiments by which scientists discovered that every </span>atom<span> contains a nucleus where its positive charge and most of its mass are concentrated. They deduced this by measuring how an </span>alpha particle<span> beam is scattered when it strikes a thin metal foil. The experiments were performed between 1908 and 1913 by </span>Hans Geiger<span> and </span>Ernest Marsden<span> under the direction of </span>Ernest Rutherford<span> at the Physical Laboratories of the </span>University of Manchester<span>.</span>
Answer:an element (e.g. arsenic, antimony, or tin) whose properties are intermediate between those of metals and solid nonmetals or semiconductors.
Explanation:
Answer:
1.2 × 10⁴ cal
Explanation:
Given data
- Initial temperature: 80 °C
We can calculate the heat released by the water () when it cools using the following expression.
where
c is the specific heat capacity of water (1 cal/g.°C)
According to the law of conservation of energy, the sum of the heat released by the water () and the heat absorbed by the reaction () is zero.
Answer:
1.626 M
Explanation:
Let's start by <u>calculating how many grams of C₂H₆O₂ are there per mL of solution</u>:
- 1 mL of solution weighs 1.40 g.
- 1.40 g of solution * =0.1008 g C₂H₆O₂
So the C₂H₆O₂ concentration can be expressed as 0.1008 g/mL.
Now we <u>convert g/mL to molarity</u>, using the <em>molar mass of C₂H₆O₂:</em>
- 0.1008 g C₂H₆O₂ ÷ 62 g/mol = 1.626x10⁻³ mol C₂H₆O₂
(1 mL = 0.001 L)
- 1.626x10⁻³ mol C₂H₆O₂ / 0.001 L = 1.626 M