<h3>
Answer:</h3>
272.43 K or -0.718°C
<h3>
Explanation:</h3>
We are given;
The initial pressure,P1 as 761 mmHg
Initial temperature, T1 as 0.00°C which is equivalent to 273.15 K
Final pressure as 759 mmHg
We are required to calculate the final temperature;
According to pressure law, the pressure of a gas and absolute temperature are directly proportional at constant volume.
That is; Pα T
Therefore, at varying pressure and temperature,

To get final temperature;



Therefore, the final temperature will be 272.43 K or -0.718°C
Answer:
Choices 2 and 4
Explanation:
HCL is formed witthe the elements Hydrogen and Chlorine. Whatever is on the left side of the equation must match up with the right side of the equation.
2. H + Cl --> HCl (we have one hydrogen and one chlorine)
4. 2HCl --> H2 + Cl2 (since the two is distributed to both the H and the Cl, H has 2 and Cl has two on the left side AND on the right side of the equation)
If 14 grams of hydrogen reacted with 24.7 grams of oxygen 27.7875 grams of water will be formed.
Explanation:
2H2+O2----------->2H2O.
- From the above equation, we can say that 4g of Hydrogen will react with 32 g of oxygen.
- In this question, Hydrogen is in excess amount.
- 32 g of Oxygen will react with = 4 g of H2.
- Therefore 24.7g of Oxygen will react with =24.7x4/32= 3.0875 g H2.
- The remaining 10.9125g of H2 will be left unreacted.
- Therefore the amount of water formed=(24.7+3.0875)=27.7875 g
Answer:
Ionic Bond
Explanation:
The atom with the higher electronegativity wants to fill its valence electron shell (meaning it wants 8 electrons in this shell). The atom with lower electronegativity will want to empty <em>or donate </em>an electron so that it can have an empty valence shell.
Answer:
Eventually, these individual laws were combined into a single equation—the ideal gas ... We find that temperature and pressure are linearly related, and if the ... then P and T are directly proportional (again, when volume and moles of gas are ... of the variables, and they are more difficult to use in fitting theoretical equations ...
Explanation: