Answer:
Its chemical formula is NaHCO3. Its formula consists of one sodium (Na) atom, one hydrogen (H) atom, one carbon (C) atom and three oxygen (O) atoms.
Explanation:
Hope this helps
Answer:
23.8 L
Explanation:
There is some info missing. I think this is the original question.
<em>Calculate the volume in liters of a 0.0380M potassium iodide solution that contains 150 g of potassium iodide. Be sure your answer has the correct number of significant digits.</em>
<em />
The molar mass of potassium iodide is 166.00 g/mol. The moles corresponding to 150 grams are:
150 g × (1 mol/166.00 g) = 0.904 mol
0.904 moles of potassium iodide are contained in an unknown volume of a 0.0380 mol/L potassium iodide solution. The volume is:
0.904 mol × (1 L/0.0380 mol) = 23.8 L
Secretary of State John Hay sent his Open Door Notes (1899-1900) to world powers to protect United States trading interests in China. The correct option among all the options that are given in the question is option "3". These notes were mainly in regards to providing equal opportunity for trades in China and also respecting China's sovereignty, territorial integrity and administration. The principles of operating in China was the same for the British as well as for the United States, but John Hay was the first person to give it a written form. After this the official policy of the United States was based on the written document during the first half of the 20th century.
Answer:
1.72x10⁻⁵ g
Explanation:
To solve this problem we use the PV=nRT equation, where:
- R = 0.082 atm·L·mol⁻¹·K⁻¹
- T = 25 °C ⇒ (25+273.16) = 298.16 K
And we <u>solve for n</u>:
- 1 atm * 5.7x10⁶ L = n * 0.082 atm·L·mol⁻¹·K⁻¹ * 298.16 K
Finally we <u>convert moles of helium to grams</u>, using its <em>molar mass</em>:
- 4.29x10⁻⁶ mol * 4 g/mol = 1.72x10⁻⁵ g
In my opinion, the best answer among the choices listed above is the first option. The major reason for chemical bonding is <span>for atoms to gain the stability of the octet. In general, chemical reactions happen in order for substances achieve stability or appropriately achieve equilibrium.</span>
